experiment rusting of iron nail

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Rusty nail experiment

Follow FizzicsEd 150 Science Experiments:

You Will Need:

• 6 Test tubes or plastic cups
• 6 Steel nails (avoid galvanised ones)
• Lemon juice
• Cooking oil.
• Optional: Saltwater, detergent.
• Adult supervision

• Instruction

Set up the 6 test tubes or cups as shown in the picture above. This experiment is very much about  variable testing !

Take a photo and write down your observations of each nail at the start of the experiment. This is also a good time to enter this into your own  classroom blog !

Optional: Weigh each nail with an accurate scale at the start and the end of the experiment.

Optional: Try different nails in the same liquid… do they rust differently?

Over the coming days take recordings of each nail’s condition.

– Which nail showed rust first? – If you were able to weigh each nail at the end of the experiment, was there any difference between the nails? Why?

This setup is just one way of running this classic rust experiment. You could also try the following experiment conditions too:

• nail completely submerged in water vs. half submerged.
• nail completely submerged in water with a layer of oil over the top of it.
• nail in salt water vs. nail in pure salt

You could also try normal steel nails vs. steel wool to investigate the effect of surface area on rusting rates as well.

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Why Does This Happen?

Rusting is the oxidation of metal, whereby the oxygen in the environment combines with the metal to form a new compound called a metal oxide. In the case of iron rusting, the new compound is called iron oxide… also known as rust!

This science experiment is all about controlling variables to explore which material will rust an iron nail first.

Variables to test

More on variables here

• Try boiling the water… does this make the nail rust faster, slower or is there no impact on the rusting time?
• What happens when you use different liquids?
• If you scratch the nail first, will it rust faster or slower?
• What if you use iron wool and iron filings instead?
• Try galvanised nails

Further information

Rusting, also known as corrosion, is the reddish-brown layer formed over an iron when exposed to air and water. Rusting occurs mainly because of a chemical reaction between iron with water and oxygen in the air.

Simple formula…     

Water + Oxygen + Iron = Rusting

The chemical reaction usually occurs very slowly and it is an oxidation process. Rusting can also occur on other metals such as copper and they may not always be called ‘rust’.

Rusting can also occur in water. The carbon dioxide gas in the air mixes with water to form a weak acid called carbonic acid. This acidified water can dissolve some of the iron and water begins to break down into oxygen and hydrogen. The free oxygen reacts with the dissolved iron to form iron oxide or rust.

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27 thoughts on “ Rusty nail experiment ”

How many day will nail rust in tap water,vinegar,salt water, sprit and cooking oil

Hi Kolwawole! Thanks for your question. The time to rust for the nail is highly dependent on the liquid the nail is immersed in. In water, you tend to see the beginnings of rust within a couple of days or so whereas other liquids take longer. Try the experiment out and let us know your results!

I bought non galvanised steel nails (they are called bright steel) and I have had them in my liquids (salt water and tap water) for a week now and instead of showing signs of rust they have just gone a grey colour. Do you know why? How can I adjust the experiment to make them actually rust? Thanks

Interesting! It looks like that if your nails were non-galvanised, it would have been to do with dissolved minerals such as carbonates in your water. The more carbonates, the ‘harder the water’. The harder the water the more difficult it is to rust a hot-dip galvanised nail as it affects the pH and the action of sodium and chlorine ions that come from the dissolved salt in the water ( see this link ). The thick layer of Chromium and Zinc on the galvanised steel slows the rusting as it prevents oxygen reaching the metal (at least for a while). You can actually see this affect by scratching off part of the galvanised layer and then letting this area rust as you’ve removed the protection ( read up on crevice corrosion ).

The thing is, your bright steel nails are non-galvanised. This means they should have little to no protection to the salt. If left for longer, the nails should begin to corrode on the outside. The rust formed on the outside is still permeable by the water and salt ions, which means that we would expect this rusting to happen underneath the top layer of rust as well. This should continue until the nail becomes completely iron oxide (rust). Let us know if this happens! For full details on the chemistry of nails rusting, check out csun.edu.

Thanks for your question!

I’m really confused about how can I weigh corrosion in metals. Can you please help.

Hi Rouzana! If you are able to have access to laboratory scales within a high school, you should be able to take a measurement of each nail mass before and after the experiment. The more sensitive the scales, the better!

hi can you please tell me the aim and the hypothesis of this experiment. thanks

Hi! Here’s something that could start you off; – Aim; To determine which liquid produces the most rust on an iron nail. – Null Hypothesis; There will be no change in rust on an iron nail when immersed in ‘ABC liquid’. Have fun!

Hi! Do you know what type of reaction this and also the science behind it? Thank you!

Hi Lara! This is an example of a Redox reaction, wherein this case the iron reacts with water and oxygen to form hydrated iron(III) oxide, which we see as rust. See further details here!

I wanted to do a variation of this experiment for my high school class. Instead of weighing the change in mass to determine the amount of oxidation, I was wondering if there was a chemical that could dissolve only the nail(iron or any other metal) leaving the remaining iron oxide behind.

Sorry Michelle, I’m not sure of a chemical that will do this. If you find out please let us know!

hey can you tell us the chemical formula of the equation iron+water+oxygen= hydrated iron(III) oxide Should we cover the bottle of water to hasten the rusting process ? thank you

Hi Viv! There’s actually a few things going on here over three separate reactions: A great summary of the three reactions can be found here The final balanced equation is below, however this covers both Fe(II) and Fe (III) ions. 4Fe + 3O 2 + 6H 2 O → 4Fe(OH) 3

If I have four solutions (water, salty, bleach and with oil) which will corrode the fastest? the slowest?

Hi!, I placed screws/nails in vinegar and lemon juice and after 9 days they turned black, I was wondering what is the cause of this?

Hi! The acid from both liquids removed the outer coating and exposed the underlying metal to the air which caused oxidation

hi, I have a doubt, I used the ss steel screw ( nail) and I kept them in vinegar, cooking oil & lemon juice. But when I checked it in the next day the screw in the vinegar turned silver to black. The same happened the same but it happened to the lemon juice

Hi! Both the vinegar & lemon juice are acids that removed the coating and allowed the underneath to oxidise.

What is their rate of corrosion (Reaction)? thank you

Hi! This is dependent on the concentration of the acids and the temperature

what are the factors that affect/speeds-up corrosion?

Solution concentration & type as well as temperature. Isolate a variable and see which make the greatest effect!

what liquid makes nails/screws rust the fastest?

Hi Piper! Please try the experiment to find out and let us know!

Do you know what are the independent, dependant and controlled variables in the experiment.

Hi! Please have a read of this article to help you with this answer 🙂 https://www.fizzicseducation.com.au/articles/variables-teaching-the-heart-of-science-experiments/?recaptcha_response=

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Science Project on Nails That Rust

Chalk and Vinegar Science Projects

If you ever wonder why nails rust, it's because rusting happens when a metal is exposed to oxygen. The "rust" is actually iron oxide and forms when the iron in the nail reacts with the oxygen in the air or in liquids. The molecules of iron on the surface of the nail exchange atoms with the oxygen in the air and produce a new substance, the reddish-brown ferrous oxide, a.k.a. rust. A simple science project tests the effects of different liquids on the rusting process, such as oil, water, vinegar and detergent.

TL;DR (Too Long; Didn't Read)

The rusting process of a nail speeds up considerably when it is in certain types of liquids. Water removes electrons from iron, leaving it positively charged. Oxygen then reacts to the positively charged iron and creates ferrous oxide. Salt water is an electrolyte, which contains charged atoms. Charged atoms cause iron to lose electrons more readily and allow oxygen to bind with the iron more freely, which accelerates rusting.

Things You'll Need

Place numbered test tubes or cups in a line to let you compare the effects of different liquids on your nails. Before you begin your experiment, take a photograph of each nail. You may also weigh each nail at this point. Place one nail in each test tube or cup.

Add a different liquid to each test tube or cup. For example, if you have six containers you could add cooking oil, tap water, vinegar, lemon juice, salt water and detergent. Write down what liquid is in each container. Over several days, take regular notes on each nail's condition. Record which nail showed rust first.

Repeat the above steps, but this time try different conditions. For example, you could compare a nail completely submerged in water to a nail only half submerged in water, or observe a nail completely submerged in water with a layer of oil on the top of it. You could compare a nail in salt water and a nail in pure salt.

At the end of your experiment, remove the nails from their containers. Weigh them to determine whether there is any difference between them.

Wear safety goggles and gloves at all times. If you use bleach or stronger acidic substances in your experiment, have adult supervision.

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• California State University: Rusting Rates of Iron Nails
• University of Illinois at Urbana-Champaign: Q & A: Rate of Rust Formation
• UCSB ScienceLine: Does Saltwater Affect the Production of Rust?

About the Author

Claire is a writer and editor with 18 years' experience. She writes about science and health for a range of digital publications, including Reader's Digest, HealthCentral, Vice and Zocdoc.

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Science At Play: Instant Rust

• Nick Villagra
• November 10, 2020

I’m sure this is something we have all experienced before- you go outside and find a tool or other metal item completely discolored. You may already know, this discoloration is called rust. We typically expect something to take weeks or months to rust, but today I am going to show you a way you can rust a nail in just seconds. Want to see how it works, and how you can try this at home? Watch the video below to learn more.

Materials to Collect

• An iron nail (Make sure it’s not galvanized)
• A plastic or glass container that is large enough to hold your nail & all of the liquid ingredients. *Do not use a metal container or it might rust too* 
• 8 teaspoons hydrogen peroxide (3%) (you can pick this up at any store where they sell first aid supplies)
• 1 teaspoon distilled white vinegar
• Safety glasses or goggles to protect your eyes
• A pair of gloves 

Try it Out! (with adult supervision)

**Before doing this experiment, it is very important that all participants are wearing personal protective equipment (PPE): a pair of safety glasses or goggles and waterproof gloves.  A pair of safety glasses or safety goggles is ALWAYS a good idea when working with liquids that could splash in your eyes. It is also a good idea to have a pair of gloves on hand because you don’t want to have prolonged skin contact once these chemicals are combined.** 

Once you’ve collected all of your materials and have your personal protective equipment on, it’s time to start the science!

Step 1: Measure out your ingredients using the amounts listed in the materials section. If you need more solution, make sure you use 8 parts hydrogen peroxide to 1 part distilled vinegar as you measure out what you need. Then carefully combine the vinegar and hydrogen peroxide in your bowl.

**Once these liquids are combined, be careful not to touch the mixture. Putting on a pair of gloves when working with this solution is a great way to keep your hands safe.**

Step 2: Add enough salt to the mixture to saturate the solution (the same way you would make really salty water). Mix the solution together, you can use the nail if it is long enough, or you can use a wooden skewer.  If you use the nail to stir, you may see a rust color and bubbles start to appear.

Step 3: Place your nail in the container. If you’re rusting more than one nail, choose a container large enough to hold all of the nails that you want to rust. 

Step 4: Let the nail sit in the solution. Any part of the nail that is sitting in the solution will form rust on it. Keep an eye on your nail, and when you are happy with how rusty your nail has become you can carefully take it out of the solution. 

Step 5: Let the nail air-dry. Wear gloves and carefully remove the nail from the solution. If you wipe down the nail you may lose some of the rust finish. Place it gently on a paper towel and let it air dry. In a few hours, your nail should look rusty and you can check it out a little closer.  Be sure to safely drain your solution and dispose of your gloves.

What is the Science? 

So what is rust anyway?

Rust forms on metals in a process called oxidation. Oxidation occurs when certain metals, like iron, are exposed to oxygen. For some metals this happens very quickly, and for others this process is a little slower. Metals that are protected by paint and other coatings will not rust because those coatings are protecting the metal from being exposed to oxygen. If some part of the coating is removed or damaged (like a scratch on a car, or paint on a bicycle wearing off) the metal will then be exposed to oxygen and the process of rusting can begin. 

What is actually happening when rust forms?

In our experiment, mixing hydrogen peroxide (H 2 O 2 ) and distilled vinegar together creates a small amount of something called peracetic acid. Acid is corrosive and can cause things like metal to break down. Hydrogen peroxide is made of hydrogen and oxygen, but it’s the oxygen that’s key to creating rust on metal.  

The molecules of iron on the surface of the nail exchange atoms with the oxygen in the solution and produce a new substance. You guessed it–rust! (or iron oxide as scientists would call it!)

This whole process is helped along by the salt we added to the solution. Its job in this whole process is to act as an electrolyte which lowers the electrical resistance in the solution, helping the oxygen and the nail to trade atoms more easily. 

** Atoms are the pieces that make up a molecule. These are super tiny and impossible to see with your own eyes, so scientists have to use very powerful equipment to see these tiny building blocks**

Why am I noticing so many changes?

Any time you see bubbling, fizzing, or a color change, that is a clue that you’re probably seeing a chemical reaction. This means that our iron is changing. Once the nail undergoes the process of rusting we can remove the rust from the nail, but the iron that turned to rust will never go back to being iron. 

You might also notice the reaction getting warm. This particular chemical reaction is an exothermic reaction, meaning a chemical reaction that produces or gives off heat. This is one of the reasons we want to be sure to use proper tools and safety equipment throughout the entire experiment. If the nail is too warm for you to comfortably touch, use a kitchen utensil like tongs to remove your nail, or pot holders to safely relocate your container.  

Ask Your Young Scientists

As you begin combining ingredients to make your solution, ask:

• They may see and hear some fizzing, some bubbling, the salt disappearing (dissolving) into the mixture, and they may notice that the mixture is clear but gets cloudy as the salt is added 

Once the nail is in the solution, ask your scientists:

• They may see and hear more fizzing or bubbling, the color changing, they may notice that the container feels a little warmer after a few minutes, or even see rust beginning to form on the nail
• Your scientist may wonder why the color of the solution is changing, why it is bubbling, they may wonder why the solution has a different smell. They might wonder what rust actually is.

Once the nail is out and dry, ask your scientist to make a few comparisons between a rusty nail and a non-rusty nail. 

• What things are different? 
• What things stayed the same?

More to Explore

The amount of time you leave the nail sitting in the solution will determine how rusty your nail gets. If you only want a little bit of rust, try taking your nail out after a few minutes. If you want a really rusty nail, try leaving your nail in the solution all day, or maybe longer. You can leave the nail in the solution for as long as you want, but keep in mind that the container may get very warm if the nail rusts for an extended period of time.

Try this same investigation again but with a twist. Either use another nail or wipe off the nail you just used with a paper towel.  Before you put the nail into the solution try covering it in petroleum jelly.  Will it still rust? Let’s find out! 

This content was made possible in part by the Institute of Museum and Library Services.

We want to see what you try at home. share your experiments with us on social media by using the #scienceatplay and tagging @ctsciencecenter..

Nick Villagra is a STEM Educator at the Connecticut Science Center, responsible for developing and delivering science experiences, including classroom lab programs, stage shows, and vacation camps. Nick holds a Bachelor’s of Science in Engineering from Swarthmore College. and has been a speaker at the New England Museum Association conference. Always looking to put a unique stamp on the Science Center’s offerings, Nick enjoys incorporating custom-designed 3D printed materials for students to interact with.

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Source:  Declan Fleming

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By Declan Fleming 2016-03-10T00:00:00+00:00

Declan Fleming presents an experiment to illustrate the electrochemistry of rusting

Most courses studied by 16–18 year olds require them to be familiar with the process of rusting from an electrochemical perspective. However, many rusting demonstrations take a long time to produce any results without providing much information about the various electrochemical processes occurring. The use of phenolphthalein and hexacyanoferrate(III) as indicators is a rapid and great way to infer the presence of the various ions that form during rusting.

Source: © Declan Fleming

• Potassium hexacyanoferrate(III) (about 0.2 g) (skin and eye irritant, harmful if inhaled or ingested)
• Phenolphthalein indicator solution (highly flammable, eye irritant, harmful by ingestion)
• Sodium chloride (about 0.25 g)
• Four petri dishes
• Four iron nails or strips
• Non-insulated copper wire or strips (10 cm)
• Magnesium ribbon (3 cm) (flammable, releases flammable gases on contact with water)

Preparation

Work in the location of the demonstration where possible to minimise the movement of the liquid. To 100 cm 3 of tap water, add half a spatula (about 0.2 g) of potassium hexacyanoferrate(III), eight drops of phenolphthalein indicator solution and (optionally) a microspatula of sodium chloride (0.05 g) to accelerate the process a little.

Shake or stir the solution to aerate and then distribute it among four empty petri dishes to a depth sufficient to cover the nails once added. In one of the dishes, dissolve a further half a spatula of sodium chloride (about 0.2 g). Leave for a few minutes to allow the liquids to settle – in this time you can prepare the nails.

Wrap the centre of one nail with a strip of magnesium ribbon and the centre of a second with a copper strip or wire. You may wish to crimp these both slightly with pliers to improve electrical contact between the metals. Note that copper wire kept in schools often appears uninsulated while still being covered with a thin insulating layer; this can be scratched off by rubbing against a scissor blade or with an emery cloth.

In front of the class

Add one of the unmodified nails to the salty water petri dish. The remaining unmodified nail (a control) and the two modified nails can now be added to each of the other three petri dishes. Over the course of a few minutes, the phenolphthalein indicator turns pink (indicating the presence of OH – (aq)) around the magnesium-modified nail. Then over the course of an hour, the potassium hexacyanoferrate(III) turns blue around the other three nails (indicating the presence of Fe 2+ (aq)). A small amount of pink is also seen around the copper-modified nail.

Alternative methods

There are many alternatives to this experiment. Try placing the iron and magnesium in separate petri dishes and connecting them using copper wire, or repeating the experiment in boiled water under oil. What happens if a nail is placed in a large droplet such that at least one end is exposed to the air?

Although it is more time-consuming to prepare, agar gel is more forgiving of movement than water. A preparation using it can be found here .

Teaching goal

The primary objective here is for students to be able to explain the process of rusting from an electrochemical perspective. 

The hydroxide ions come from the reduction of aqueous oxygen (See Standard electrode potentials , equation 4). As magnesium is a better reductant than iron or copper (equations 1–3), the pink colour formation is fastest in the case of the magnesium-modified nail. The magnesium also pushes electrons onto the iron, improving its ability to reduce water meaning the pink colour rapidly forms around the entire nail.

No blue colour is seen here because the magnesium is preferentially oxidised, preventing oxidation of Fe to Fe 2+ . The outcome is the same whether the iron is attached directly to the magnesium or via a wire.

The copper has the opposite effect on the iron. With iron being a better reductant than copper, electrons are pushed onto the copper and a pink colour is seen around that metal. The iron is preferentially oxidised, accelerating the oxidation of Fe to Fe 3+ and therefore the blue colour (equation 5) appears around the iron. The blue appears faster and deeper here than in the salty water or control experiments.

The production of the blue colour around the nail in salty water is faster than the control due to the increased concentration of electrolyte, even though the solubility of oxygen is reduced by increased salt concentration.

Note that the depth of colour formation around these nails is not uniform. This indicates that electrons are being transferred through the nail from the site of oxidation of the metal to the site of reduction of the aqueous oxygen. Using iron nails rather than strips shows how the shaping of the metal locally increases the free energy of the iron and as such, the blue colour is often deepest around the tip of the nail.

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Wear eye protection. All liquids can be washed down the sink with plenty of water. Indicator solutions are likely made with industrial denatured alcohol (IDA). IDA is also an eye irritant, harmful by ingestion and causes damage on repeated or prolonged exposure to the optic nerve, CNS (and some other organs). Potassium hexacyanoferrate (III) is a skin/eye irritant, harmful by ingestion (and perhaps skin contact), harmful if inhaled/respiratory irritant, releases toxic gases in contact with acid.

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Corrosion experiment - Rusting nails

Corrosion of metals is an electrochemical process (Redox reaction) and fundamentally it requires 4 components:

Cathodic reaction (Reduction reaction, positive polarization): A reaction that gains electrons. As a result, the oxidation number decreases. For instance, hydrogen and oxygen reduction reactions are common in acidic and aerated solutions, respectively. The site where the cathodic reaction occurs is called the cathode.

Proton reduction reaction 

$$2{H^ + } + 2{e^ - } \leftrightarrow {H_2}(g) \tag{1} \label{eq:1}$$ 

Oxygen reduction reaction

$$ {O_2}(sol.) + 2{H_2}O + 4{e^ - } \leftrightarrow 4O{H^ - } \tag{4} \label{eq:4}$$

Anodic reaction (Oxidation reaction, negative polarization): A reaction that loses electrons. As a result, the oxidation number increases. Generally, this is the metal dissolution reaction. A metal in metallic form, which has an oxidation number of zero, loses electrons and becomes ions. Metal ions can dissolve away or further react with the surroundings, such as with oxygen to form oxides scales. The site where the anodic reaction occurs is called the anode.

Iron oxidation

$${Fe}\rightarrow{Fe^ {2+} } + 2{e^ - } \tag{5} \label{eq:5}$$ 

Zinc oxidation

$${Zn}\rightarrow{Zn^ {2+} } + 2{e^ - } \tag{6} \label{eq:6}$$ 

Electrolyte : a conductive solution to carry ions. Seawater is an effective electrolyte for corrosion due to high salt concentration. Coastal regions are thus more susceptible to corrosion than areas further in land due to deposition of salt aerosols.

Electrical conductor : an electrically conductive medium to transport electrons. For instance, an electrical wire connecting two metal pieces, direct contact between dissimilar metals, or the metal itself.

Different metals have different tendencies to corrode, thus some would corrosion more readily than others (i.e., we say they would be more anodic). In fact, local anodes and cathodes develop even on the same metal surface as they are heterogeneous. 

The dissimilar metal corrosion and the effect of heterogeneities in metals on corrosion are demonstrated using steel nails in an agar gel with a pH indicator and ferrous ion indicator. In these examples, the steel nail corrosion was accelerated when electrically connected to copper and was mitigated when connected to zinc. The time-lapse videos show colour changes as reactions proceeded.

Nail - Zinc

Nail - Copper

When it is simply just the steel nails in agar, corrosion still occurred. This is because of metal heterogeneities and cold work (bending).

Nail - straight

Nail - Bent

We developed a supplementary note to further explain science behind this experiment, some troubleshooting, and additional resources.

Kod Pojtanabuntoeng

Associate Professor

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Rusting Nails student experiment & research (cont'd)

Students (and some teachers) assume that rust is the best indication that corrosion is occurring, but it isn't! In fact, in industry, acids are used not to create rust but to remove it. Although acids can dissolve metal, they will dissolve rust faster, leaving the surface rust-free.

So what has happened is --

With your vinegar and orange juice, any rust has been dissolved into the acid. In addition, a very small amount of iron has probably also been dissolved. Steel nails are made of iron plus a small amount of carbon. As the iron dissolved, it left behind the very tiny specs of carbon because carbon is not soluble in mild acids. You will probably find out that this black "smut" can be wiped off with a tissue or paper towel. But I'd suggest wiping it off onto a coffee filter instead, so all of your corrosion products are "mounted" on coffee filters.

In the salt water, the iron from the nails combined with oxygen dissolved in the water to form iron oxide (rust). I'd suggest rubbing any rust off onto a coffee filter and pouring the liquid through the coffee filter.

The amount of rust and smut on the coffee filters should be a good measure of what happened. The ideal way to measure corrosion is by the reduction of weight of the nail between start and finish, but I doubt that you have scales of sufficient accuracy, so you may have to exhibit your coffee filters as your measurements. You can do a rough graph of how much smut and rust you see on each coffee filter. Good luck.

Q. Hi, it's me again. I am almost finished with my written report but I still don't have a hypothesis...I'm sure you're not allowed to give a hypothesis to me, but I was wondering if the hypotheses I chose is correct. My hypothesis is that the nail in the salt water will rust the fastest. I'm a little bit confused. My topic is the effects of different contaminants on the rate of rusting. So I don't think my hypotheses is right for my chosen topic. What do you think? Please help me...I really really need your help... Thank very much....

Let's take it from the top --

You don't just start an experiment with no purpose. As I noted in my response to Zoe in about the middle of this thread, Darwin himself said that this would be like going into a gravel pit every day and pointlessly writing down the size and color of each piece of gravel. There needs to be a point to your experiment, something that you are trying to prove or disprove. That "something" is your hypothesis.

The "hypothesis" that you now suggest might have been okay, but you were supposed to form your hypothesis before you began your experiment, and the purpose of the experiment was to see whether the evidence supported or tended to refute your hypothesis. The position you are in now is that you want to use your "conclusion" that salt water rusts things fastest as your hypothesis. See the problem, and why that's no good?

So let's look at it this way: when you began your experiment, you suspected that different contaminants would affect the rusting rate. You didn't know it to be a fact, you just suspected it based on intuition, previous experience, or rumors you heard, etc., right? What you wanted to do was to conduct an experiment to support or refute that suspicion. So, how about this as your hypothesis: "When nails are immersed in water-based liquids, the amount of rust that is formed will vary depending upon what contaminants are in the water they are immersed in."

So you picked a good variety of liquids (salt water, sugar water, vinegar, orange juice, and Dr. Pepper) and ran an experiment to prove this hypothesis -- and the conclusion was pretty clear: the amount of visible rust on the nails in salt water was the greatest. You also discovered that immersion in vinegar or orange juice produced a black smut on the nails. You believe that this black smut is carbon that did not dissolve in these mild acids, but you do not know that for a fact, so you suggest a good hypothesis for next year's science experiment might be: "Immersing nails in vinegar or orange juice dissolves some iron from their surface, leaving behind a carbon smut".

Q. Good day, My name is Naomi and I was assigned a rusting rate project. We also had to write a written report but I don't have a problems or specific questions to answer in my project. So far, my problems are: Which of the contaminants have the most significant effect on the rate of rusting iron nails? Which nail rusts the fastest? What properties are present in the contaminants that may have an effect on the nails? Are those related or acceptable in my topic? My topic is the effects of salt and other contaminants on rate rusting? Please I really need your help.... Thank you!

Q. Hello.... I'm in the 9th grade and I have a question about my project which is the effects of different contaminants on the rate of rusting. On the previous answers you have given, you said that you can measure the rust by rubbing the rust off the nail. How do you measure the rust that was rubbed? And as you answered in Chelsea's question, you stated that the black smut that was found in the nail in the vinegar are carbon specs left behind. I wanted to ask if it was still considered as rust?. Because that also happened in my project. PLEASE PLEASE HELP ME! I DESPERATELY NEED YOUR HELP...THANKS!

The ideal way to measure rust is to weigh the nail before you start the experiment, let it rust in the solution for your experiment, then use special chemicals to dissolve away the rust, and then weigh the nail again -- determining the amount of corrosion by how much weight of metal the nail has lost.

But depending on what grade you are in, what chemicals the school lets you use, and what equipment your school has, you probably have to compromise rather than doing it the ideal way. A compromise which is probably suitable for younger grades is to rub off any rust you can onto a coffee filter, and pour the rusty water through the same filter.  You can't actually "measure" rust this way, but I think you can "judge" the relative amount of rusting by looking at how much rust is on the filter.

I am only guessing that the black smut is carbon specs; neither of us has done an experiment that proves it. But, no, carbon is not rust. "Rust" is iron oxide, the chemical combination of iron from the nail with oxygen from the air or dissolved in the liquid.

I believe the right approach to your report is to understand the principles that we've talked about here, and describe what you've found and the limitations on what you've been able to do based on a student's limited access to chemicals and exotic testing equipment. Good luck!

Q. Hello, What I meant with the question was that in my experiment, the nail that was in the vinegar rusted the most, while in most of the research that I saw salt was supposed to rust more. I followed the procedure that was to weigh the nails before and after the experiment. But before I weighed the nails after the experiment, I cleaned the rust off to see how much weight is lost. In my project, It showed that vinegar had the most weight loss, while salt had the least weight loss. I just wanted to ask why it happened? Why was vinegar the nail that had the most rust? I really really really need your help. This project is due next week and I still don't know why the results happened. Please Please help me.....Thanks....

Q. Please help me.... I'm a ninth grader and I did a rusting project. The effects of different contaminants on the rate of rusting. The contaminants that I chose were OJ, vinegar, and salt water. The nail in the vinegar rusted the most followed by orange juice, and then salt water. I know that the vinegar is acetic acid and dissolves metal and corrodes only when it is evaporated. But I wanted to ask about salt water. why did it rusted the least? Is it bec. it has a higher pH level? Or does it have something to do with electrochem? Please help me...need a response by hpoefully tom....thank you so much....

Q. Hey ted I'm kim and µm I'm doing a science project on the effects of soda on nails and I'm using dr. pepper, coke, vanilla coke, cherry coke, water, pepsi, and sprite now I've been told that nothing will dissolve keratin nor steel nails but what are your thoughts? and also I have to do note cards with this experiment how would I get A LOT of info that can fill 50 note cards? sincerely, Kimberly Grace

Q. Hello I am in 6th grade and I am doing a science fair project on "science What liquid will make a nail rust the fastest?" my materials are: vinegar, tap water, sprite. But I need an idea for the Procedure.... Write me back as soon as you can thanks!

Q. I am a 7th grader and I need to know what the chemical reaction would be when vinegar rusts a nail. I saw the black stuff on it and want to know what it is.

Q. I have a 10 year old 4th grader that is doing a science fair project and I was never good at science and do not have all the answers to help him. I have read some of the threads and it helped me understand some to help my son understand his project, but I am left with other questions. He is doing a project on which of bleach, tap water (we have well water), or salt water would rust an uncoated framing nail the fastest. He has done the experiment twice now and has had very similar results. We found that the bleach rusted the most and quickest and I think I have gathered from some of the other threads on why as it basically has more oxygen released to cause the iron to oxidize more and quicker. I think I stated that correctly. Anyway, the tap water seemed to rust a bit more than the salt water in both of the experiments. I saw that you have done this experiment yourself and came to the conclusion that they rust about the same. My question would be why would in my sons experiments the tap water rust more than the salt water both times. He needs a reason to place with his graph he places on his poster board for the project and I have no idea on where to begin to look for an answer. My son is a straight A student which he gets from his father. lol He wants to excel and I am trying to help and I feel like someone is speaking a foreign language to me when it comes to science. My son suggested that the salt in the jar that the nail was half submerged in was preventing oxygen to be released and in turn caused less rust. I don't know if this is correct or not and don't want him looking silly with this conclusion if it's wrong. I just don't see what can be gained from this project besides him learning how to do one. He's been doing the journal and understands to get accurate results that an experiment must be done a few times to maintain the same results. But why would knowing that bleach rust something more be helpful? It's not like bridge building companies for example would have to worry about bleach getting on their bridge and corroding it.

Q. I have an experiment project in school ... but I always forget to do it ... but I just wanna ask what happens to a nail placed in a glass jar without water and uncovered? And what happens to to a nail placed in a glass jar with water and is covered? does the nail in the water or or the other forms rust on it's surface? please answer .. :)

Q. Hi, my name is genesis and I'm in the 9th grade. I'm doing a project based on rusting. I did my experiment and found that after a day of being in salt water and distilled water, nails rust faster in distilled water. Can you please explain why this happened?

Q. I helped my daughter post the following observation/request in a different post, but I am doing so here again because the topic here seems closer to her project and questions. My daughter and I will appreciate all explanations from the chemical professionals. My 11 year-old 5th grader is doing a project on which 'environment' will cause rust to form fastest. She has used 6 non-galvanized nails cleaned with rubbing alcohol and placed in 6 test tubes filled with NOTHING, RICE, TAP WATER, OIL, vinegar, and BLEACH, respectively. After nearly 7 days of observations and data recording, we have seen some expected results and some puzzling occurrences. All tubes were left at avg room temp of 70 °F and avg humidity of 40%. The tube with NOTHING had no rust to show - as expected because it would take a long time to form. The tube with RICE also showed no rust - presumably because of the hygroscopic property of rice. The tube with regular TAP WATER did show rust on the nail and lots of rust particles settled to bottom. The nail in OIL showed no rust - presumably due to the oil creating a coating around it and preventing oxygen and moisture from contacting the nail's surface. The nail in vinegar gave us a puzzle: there was no rust on the nail which was submerged in vinegar, but the surface outside of it was covered with an extremely crusty, dark reddish-brown and black substance (i presume it is rust, but it didn't look like what we saw in tap water.) The nail in BLEACH caused amazing rust-like clumps to form within a few days. We expected the rust in water, but the results in vinegar and bleach has me stumped. I don't have an explanation for my daughter as to why the submerged half of nail in vinegar is free of rust but the surface untouched by the acidic liquid is covered profusely with dark rust-like material. Nor do I know what to say about the profuse clumps of light brown rust in the tube with nail and bleach. I have read other posts having similar results, but I am not clear as to the WHY of the results. PLEASE HELP ME UNDERSTAND.

Q. I am doing an experiment on how easily galvanised iron nails go rusty compared to ordinary iron nails?

Q. hey yall listen I need help so go down keep goin can yall help me. I need facts on corrosion of a nail in Coke, Sprite and Sunkist. I am using a steel nail. keep goin you have reached the end bye-bye' y'all want a cookie? ps. I'm in the 5th grade

Q. I am doing a science project on how does the acidity of a solution affects the rate of oxidation of an iron nail. I really need help on my procedures.

Q. I am a 7th grader doing a project on rusting nails. I need to know what the variables are for rusting nails. If you find anything please let me know. Thanks.

Dependent vs. independent variables

I am a parent helping a 4th grade student with the rusting nails science fair project. We need to list independent and dependent variables. I am just at my wit's end trying to understand the difference. HELP!! And, how can I know the difference between the two? Can you share a possible resource to help me with this confusion?

Does temperature affect the time it takes for iron to rust?

chemistry pd lab topic: corrosion race problem: plan and design an experiment to see which nail would rust faster (ordinary iron nail or galvanised nail).

Q. What happens to an iron nail after three days in sugar water?

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Rusting of Iron ( Edexcel IGCSE Chemistry )

Revision note.

Chemistry Lead

Rusting of iron

Investigating rusting.

• Oxygen  and  water  must be present for rust to occur
• You can investigate the conditions needed for rusting by setting up a series of control test tubes as shown below
• Boiled water removes any dissolved oxygen and calcium chloride is a drying agent 

Diagram showing how the conditions for rusting can be investigated

• It is in contact with both air (which contains oxygen) and water
• It is not in contact with air because the oil provides a barrier to prevent oxygen diffusing into the boiled water
• It is not in contact with water because calcium chloride absorbs any water molecules present due to moisture
• The results show that   both   air and water must be present for rusting to occur

Damage to Iron Structures

• Rust is a soft solid substance that  flakes  off the surface of iron easily, exposing fresh iron below which then undergoes rusting
• This means that over time all of the iron rusts and its structure becomes weakened

Rust prevention

Barrier methods.

• Rust can be prevented by coating iron with barriers that prevent the iron from coming into contact with water and oxygen
• However, if the coatings are washed away or scratched, the iron is once again exposed to water and oxygen and will rust
• Unlike some other metals, once iron begins to rust it will continue to corrode internally as rust is porous and allows both air and water to come into contact with fresh metal underneath any barrier surfaces that have been broken or scratched
• Common barrier methods include:   paint ,   oil ,   grease , and   electroplating

Sacrificial Protection

• Iron can be prevented from rusting using the   reactivity   series
• A   more   reactive metal can be attached to a   less   reactive metal
• The more reactive metal will oxidise and therefore corrode first, protecting the less reactive metal from corrosion
• Zinc is more reactive than iron therefore will lose its electrons more easily than iron and is oxidised more easily
• For continued protection, the zinc bars have to be replaced before they completely corrode

Zinc bars on the side of steel ships

Diagram to show the use of zinc bars on the sides of steel ships as a method of sacrificial protection

Galvanising

• Galvanising   is a process where the iron to be protected is coated with a layer of zinc
• This can be done by   electroplating   or dipping it into molten zinc
• ZnCO 3   is formed when zinc reacts with oxygen and carbon dioxide in the air and protects the iron by the barrier method
• If the coating is damaged or scratched, the iron is still protected from rusting by   sacrificial   protection

Corrosion and rusting are not the same process. Corrosion is the general term used to describe the degradation of metal surfaces whereas rusting is the specific type of corrosion that happens to iron.

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In this explainer, we will learn how to explain the conditions necessary for rusting and learn how to write balanced equations for the key reactions involved.

Rust is a reddish-brown substance often found on the surface of old or abandoned metal, such as an old car, can, or nail.

Rust is a form of corrosion that builds up over time on iron or iron alloys when they are exposed to oxygen and water. Before learning about the chemical formation of rust, let’s take a look at its physical properties.

The formation of rust can reduce the strength and stability of an iron object because of the difference in physical properties between iron and rust. An engineer that uses an iron beam in a structure will want it to remain a strong, durable, and dense beam instead of one that will expand, crack, and chip away.

In order to prevent rust, engineers can use coatings, such as oil, paint, or other metals, to prevent the surface of the metal from making contact with water and oxygen in the surroundings. They can also select rust-proof alloys such as stainless steel.

Example 1: Identifying Methods That Prevent Rusting

Which of the following suggestions is not a viable method of slowing or preventing rusting?

• Plating with tin
• Soaking in salt water
• Covering with plastic
• Coating with grease

Most of these answer options slow or prevent rust from forming. The question is asking us to find the one option that does not slow or prevent rusting.

Rust forms when iron is exposed to oxygen and water. In order to prevent rusting, we need to prevent the exposure of iron to oxygen and water.

Knowing this, one option leaps out as different: soaking in salt water certainly does not limit the exposure to water. Also, since there is oxygen dissolved in water, it does not limit the exposure to oxygen either.

The other four options—painting, plating, covering, and coating—all involve protective layers that prevent iron from contacting water and oxygen.

The correct answer is option C, soaking in salt water.

Definition: Rust

Rust is a flaky, reddish-brown hydrated iron(III) oxide formed through the oxidation of iron in the presence of oxygen and water. It has the chemical formula F e O H O 2 3 2 ⋅ 𝑛 .

Definition: Corrosion

Corrosion is the gradual destruction or damage caused by a slow, irreversible, and spontaneous redox reaction between the surface of a substance and the environment.

Note that all rust is corrosion, but not all corrosion is rust. Other metals can oxidize or otherwise corrode to form various compounds, but only iron will form the compound we call “rust.”

Chemically, rust is hydrated iron(III) oxide, with the chemical formula F e O H O 2 3 2 ⋅ 𝑛 . The “ 𝑛 ” signifies that the number of water molecules in the compound can vary.

The simplified reaction for the formation of rust is: 4 F e + 3 O + 2 H O 2 F e O 2 H O 2 2 2 3 2 𝑛 ⋅ 𝑛

This overall reaction shows that iron combines with oxygen and water to form a hydrated oxide. However, to understand the chemical process in more detail, let’s look at the intermediate reactions.

The first step is the oxidation of iron to iron(II) ions, as shown by the following half reaction. Oxidation is the loss of electrons, and this formation of ions happens as the solid iron becomes a solution: F e ( ) F e ( ) + 2 e s a q 2 + –

In the corresponding half reaction, oxygen is reduced, accepting electrons from the reaction above in the presence of hydrogen ions to form water: 4 e + 4 H ( ) + O ( ) 2 H O ( ) – + 2 2 a q g l

As well as reacting to form water, the hydrogen ions and the dissolved oxygen in the water further oxidize iron(II) ions into iron(III) ions: 4 F e ( ) + 4 H ( ) + O ( ) 4 F e ( ) + 2 H O ( ) 2 + + 2 3 + 2 a q a q a q a q l

The iron(III) ions combine with water to form iron(III) hydroxide: F e ( ) + 3 H O ( ) F e ( O H ) ( ) + 3 H ( ) 3 + 2 3 + a q l s a q

Finally, the iron(III) hydroxide dehydrates to form hydrated iron(III) oxide with chemical formula F e O H O 2 3 2 ⋅ 𝑛 .

In summary, iron dissolves in water to form iron(II) ions that are then oxidized into iron(III) ions. Hydrogen ions are absorbed, and water is produced along the way. The iron(III) ions then combine with water to make iron(III) hydroxide, which then forms hydrated iron(III) oxide.

With this process in mind, we can take a look at some of the factors that might increase the rate of rusting of a piece of iron. The simplest way to affect the rate of reaction is to change the exposure to the two main reactants, water and oxygen. For example, if we coat the iron in grease so water and oxygen cannot reach it, no rust will develop. Conversely, if we leave an iron object outside in the rain for many days, it will rust more quickly than if it is kept dry.

The iron in objects near the sea, such as boats and chains, also tends to rust quite quickly, as can be seen in the photo below. Interestingly, exposure to salt water increases the rate of rusting compared to fresh water. The oxidation–reduction reaction at the beginning of the rusting process requires the movement of electrons. The ions present in salt water make it a more effective electrolyte than fresh water, allowing electrons to be transferred more easily and rust to form more quickly.

It is worth noting that even underwater iron can rust as there is oxygen dissolved in the water. The rust can clearly be seen in the following photograph of a propeller from a Japanese ship that was sunk during the second world war.

However, if we took water and boiled it to remove the dissolved oxygen, that water would not cause a piece of iron to rust.

Other reactants in this process are hydrogen ions. Hydrogen ions are absorbed during both the reduction of oxygen and the formation of iron(III) ions, so an increase in the concentration of hydrogen ions will speed up these processes. In addition, the hydrogen ions increase the electrical conductivity of the solution, so the electron transfer in the redox reaction happens more quickly.

Acid rain can also erode protective coatings, allowing the process of rusting to begin on the iron underneath. For these reasons, an acidic environment with a low pH will cause iron to rust more quickly.

Example 2: Describing the Effect of Salt on Rusting Processes

Rusting of iron is an example of a redox reaction. The rate of rusting of iron in water varies with increasing salt concentration.

• Oxygen atoms
• Hydrogen atoms
• The rate increases because dissolved ions aid the decay of metal nuclei.
• The rate increases because dissolved ions aid the movement of electrons.
• The rate decreases because dissolved ions aid the ionization of water.
• The rate decreases because dissolved ions react with dissolved oxygen.
• The rate increases because dissolved ions react with the metal atoms.
• Oxidizing agent
• Reducing agent
• Electrolyte

This question is asking about the process of oxidation. Oxidation–reduction reactions involve the transfer of electrons from one compound or element to another. Oxidation involves a loss of electrons, while reduction involves a gain of electrons. During oxidation, iron gives up electrons to form iron 2+ ions. So, the correct answer to this part of the question is “electrons.”

This question is asking how and why salt changes the rate of reaction of rusting. To answer this question, we need to determine whether it increases or decreases the rate of reaction and the mechanism behind that change.

Part of the correct answer is that increasing salt concentration increases the rate of rusting. Iron that is either near salt water, or areas where roads are salted, rusts relatively quickly compared to metals in other environments. We can eliminate options C and D from consideration.

Next, why does salt increase the rate of reaction for rusting? As we mentioned in the first part of this question, the oxidation–reduction reaction that occurs at the beginning of rusting involves the transfer of electrons. The faster those electrons can move, the quicker the reaction will occur. In a salt solution, the electrons can move faster. Looking at the answer options, this fits with option B, the rate increases because dissolved ions aid the movement of electrons.

Option A describes the decay of metal nuclei, but radioactive decay is not involved in the rusting process. Option E suggests that the rate increases because of a reaction between the metal atoms and salt ions, but during rusting, the metal atoms react with the water and the oxygen in the solution, not the salt ions.

So, the correct answer is option B, the rate increases because dissolved ions aid the movement of electrons.

This question is asking us to define the role of salt in the rusting process.

Salt cannot be the oxidizing or reducing agent, as it does not accept or donate electrons in the oxidation–reduction reaction.

While some salt solutions can be acidic or basic, the function of the salt in this case is not as an acid or a base. Any salts will increase the rate, not just those that dissolve into hydrogen ions or hydroxide ions.

In the previous part of this question, we determined that the purpose of the salt is to aid the movement of charged particles through the solution. A substance that allows the movement of charged particles is called an electrolyte. Option E, electrolyte, is the correct answer.

The industry and manufacturers are very concerned about the risk of rusting. This concern is due to the widespread use of steel and the detrimental effects that rust has on the properties of iron. These negative effects impact the properties of the metal much more significantly than corrosion in many other metals.

Rust is the specific name for hydrated iron(III) oxide formed during the corrosion of iron, but there are other metals that corrode to form oxides as well. For example, aluminum corrodes in the presence of oxygen in the following reaction: 4 A l ( ) + 3 O ( ) 2 A l O ( ) s g s 2 2 3

Aluminum can corrode in other ways, such as in the presence of a chloride, but this way is the most common. We can compare and contrast rust with aluminum oxide to better understand the negative effects of rusting.

Patches of rust can easily chip away after they have formed, exposing more iron to be rusted; however, aluminum oxide does not chip away easily. The oxide coating on aluminum forms very quickly, resealing the aluminum if the surface is scratched or chipped.

Another negative effect of rusting is the fact that iron expands when it corrodes into rust, while aluminum contracts when forming aluminum oxide. These two physical characteristics make rust a much more disruptive oxide for machines and structures. Aluminum oxide will form a thin, dense layer on the outside of the metal that will not noticeably affect its volume. However, rust expands as freshly exposed metal deeper in the metal begins to rust.

Rust has a much more significant effect on the properties of iron than corrosion in other metals. The fact that rust can chip, cause the object to expand, and penetrate deep into the piece of metal shows the significant negative effects that need to be mitigated. Depending on the use of the piece of iron and the time and severity of the rust, the strength of the piece of iron can be compromised, making it unfit for purpose.

Example 3: Identifying Differences Between the Oxidation of Iron and Aluminum

Why does rusting affect iron more than aluminum?

• Aluminum oxides are less soluble than iron oxides.
• Aluminum is less reactive than iron.
• Aluminum oxides are less stable than iron oxides.
• Aluminum is protected by a surface oxide layer.
• Aluminum binds to water less strongly.

This question is asking us to identify a key difference between the oxidation of iron and aluminum. This oxidation process can happen when the metal is exposed to water and air. One reason why the oxidation of iron causes significant changes is that the rust can chip away. When it chips, more iron is exposed that can then rust as well.

The reason aluminum is not as affected by oxidation is that aluminum oxide does not chip. Instead, it forms a thin coating on the outside of the metal. Aluminum is more able to hold its shape and strength when it oxidizes. The correct answer is option D, aluminum is protected by a surface oxide layer.

To be thorough, we can take a look at the other options as well. Aluminum oxide and rust are equally insoluble, so option A is incorrect. Aluminum is more reactive than iron and its compounds are more stable as a result, so options B and C are incorrect as well. Option E is insignificant, as water molecules do not readily bind with aluminum molecules due to the strong oxide coating.

Different sets of conditions cause rust to form at different speeds. We can use a simple experiment to demonstrate which combinations of conditions cause rusting to happen most quickly.

Demonstration: The Effect Different Conditions Have on the Formation of Rust and the Rate of Rusting

• Place an iron nail into five separate test tubes.
• Set up different conditions for each test tube as shown in the image below.

Observation

The iron nail in test tube E will begin to rust first, followed by the iron nails in test tubes C, B, and A. The iron nail in test tube D should be the last to start rusting.

Explanation

Rust occurs when iron is exposed to both water and oxygen. In test tube D, the iron nail is placed into dry air where no oxygen is present. The anhydrous calcium chloride removes any remaining water that might be present. The iron nails placed into test tubes A and B contain either water or oxygen, but not both. So, here, rusting will be slow to occur. The iron nail in test tubes C and E are exposed to both oxygen and water. However, test tube E contains salt water, and since the presence of ions increases the rate of rusting, then the iron nail in C will rust more slowly than the iron nail in E.

• Rusting occurs quickest when iron is exposed to salt water and oxygen.
• Rusting occurs slowest when iron is protected from water and oxygen.

Example 4: Identifying the Necessary Conditions for the Rusting of Iron

Iron nails are placed into three sealed bottles containing different materials, as shown.

• 1, 2, and 3

Rusting occurs when iron is exposed to both water and oxygen. In order to answer this question, we must identify the different conditions in each of the bottles. All three bottles are sealed; however, there is still air, which contains oxygen, present inside.

In bottle 1, the iron nail is placed into boiled water with air being present. The importance of using boiled water is that boiling will reduce the amount of oxygen gas present in the water. However, oxygen from the air will dissolve into the water, and so the iron nail will likely be exposed to oxygen and water. So, rusting is likely to occur.

In bottle 2, the iron nail is again placed into boiled water. However, the water is covered with a layer of oil that will prevent oxygen from the air from dissolving in the water. Even though the iron nail is in the water, the lack of oxygen present means that rusting is unlikely to occur.

In bottle 3, there is no water present, only air and some calcium chloride. The air might contain both oxygen and water vapor; however, the calcium chloride will remove moisture from the air. As a result, the iron nail in bottle 3 is exposed to oxygen from the air, but not to water. Therefore, rusting is unlikely to occur.

Since rusting is likely to only occur in bottle 1, the correct answer is option A.

The calcium chloride in bottle 3 will remove any moisture that is present in the air. During this process, the anhydrous calcium chloride will form a hydrated salt according to the following equation: C a C l ( ) + H O ( ) C a C l H O ( ) 2 2 2 2 s l s 𝑛 ⋅ 𝑛

This reaction is not oxidation or reduction, so we can exclude options A and B. The calcium chloride is not dissolving in a solvent and therefore is not acting as an electrolyte, so we can conclude that option E is not correct.

Calcium chloride is not involved in the process of rusting and, as there is no other chemical reaction occurring, it is not acting as a catalyst.

This means that calcium chloride is acting as a desiccant. A desiccant is a substance that can induce a state of dryness, often by absorbing water. The correct answer is option C, desiccant.

• Rust is a reddish-brown substance that forms when iron is exposed to water and oxygen.
• Rust is weaker, more brittle, and less dense than iron, so the formation of rust can negatively impact iron objects and structures.
• The chemical formula for rust is F e O H O 2 3 2 ⋅ 𝑛 .
• The formation of rust is a multi-step process wherein dissolved iron ions combine with water to make iron(III) hydroxide, which then dehydrates into rust.
• Rusting occurs more quickly when there is increased exposure to oxygen or water. It also occurs more quickly when the iron is exposed to salt water or an acidic solution.
• Rust is particularly harmful when compared to other oxides, such as aluminum oxide, as it will expand and crack more as well as chip away to corrode further.

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Experiment: Investigating the rusting of iron

Experiment: investigating the rusting of iron- updated 2024.

Investigating the rusting of iron

ZIMSEC O Level Combined Science Notes: Experiment: Investigating the rusting of iron

Aim:  Investigating the rusting (oxidation) of iron

Materials:  4 iron nails, 1 steel nail, a piece of copper/brass, 5 test tubes, cotton wool, solid calcium chloride, magnesium ribbon

• Half fill two test tubes with water
• Put an iron nail in one test tube and label it A and a steel nail in another tube label it B
• Put an iron nail in a dry test tube and label it C and plug with a small piece of cotton wool on which a few pieces of calcium chloride are placed.
• Calcium chloride is a drying agent
• Wrap a piece of magnesium ribbon around and an iron nail and put it into the fourth test tube and label it D fill it with water
• Half fill the remaining test tube with boiled water. Put an iron nail with a layer of oil to exclude air and label the tube E
• Leave the test tubes for a few days and observe the results

Results and Observations

• The iron nail in test tube A will be covered with a layer of rust after a few days
• There is very little if any rust on the steel nail in test tube B
• There is no rust observed on the iron nail in test tube C
• There is no rust/little rust on the iron nail in test tube D
• There is no rusting on the iron nail in test tube E
• Iron is susceptible to rusting
• Rusting can only occur in the presence of moisture (water) and air
• Controlling humidity ( test tube C) prevents rusting
• Galvanising using a more reactive metal such as zinc prevents the rusting of iron
• Oiling reduces/prevents rusting

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• Chemistry Practicals
• CBSE Class 9 Chemistry Practical
• Class 9 Practical Experiment on Reaction of Iron With Copper Sulphate Solution in Water

Experiment on Reaction of Iron with Copper Sulphate Solution in Water

A physical change occurs when there is no change in the composition of a substance and no change in the chemical nature of the substance.

The interconversion of state occurs during physical change.

SOLID ⇄ LIQUID ⇄ GAS

A chemical change is a change that causes a change in the chemical properties of matter, resulting in the formation of a new substance. As an example, consider the burning of oil or fuel.

Heat is evolved or taken in, the formation of bubbles, gas, and fumes, as well as a change in the colour of the reactants, can take place when they form a product.

Reactants → Products

A + B → C (Chemical reaction)

Table of Contents

Materials required.

• Observation

Precautions

• Frequently Asked Questions – FAQs

To carry out the reaction between Copper sulphate solution and water and Classify it as physical change and chemical changes.

Iron nails, Copper Sulphate solution, Test Tube, Clamp Stand, Sandpaper.

The colour of pure iron is greyish. Pure copper is a reddish-brown metal. The presence of Cu2+ ions causes the aqueous C solution of copper sulphate to be blue. The presence of Fe2+ ions causes the aqueous solution of ferrous sulphate to be pale green.

Since iron is more reactive than copper, it removes copper from its salt solution.

2. Separate two test tubes and label them A and B. Add 10 mL of freshly prepared copper sulphate solution to each test tube and secure these test tubes in two separate clamp stands.

3. Thread the nail and hang it in test tube B. It is important to ensure that the iron nail is completely immersed in CuS0 4 solution. Tie the other end of the thread to the stand.

4. Keep the other iron nail on a piece of white paper.

5. Leave the setup alone for a while.

6. Take the nail out of the solution and place it along the side of the second iron nail on the sheet of paper.

7. Record your observations.

Observations

1. The brown coating on the iron nail indicates that copper is deposited on the iron nail as a result of iron displacement.

2. The colour of the blue colour copper sulphate solution changes to green.

3. The greenish colour of the solution in the test tube indicates the presence of Fe 2+ ions in the solution.

4. This is a single displacement reaction in which copper is displaced by iron from copper sulphate solution, resulting in the formation of a new compound, ferrous sulphate.

5. A chemical change occurs as a result of the reaction.

1. Clean iron nails by rubbing with sandpaper.

2. Copper sulphate solution is poisonous, so use caution when handling it.

3. The test tubes should not be touched or disturbed during the experiment.

4. After completing the experiment, the copper-coated iron nail should not be touched.

Frequently Asked Questions on Reaction of Iron with Copper Sulphate Solution in Water

What is the colour of copper sulphate solution.

The colour of the copper sulphate solution is blue.

Why are iron nails rubbed with sandpaper?

Iron nails are rubbed with sandpaper so as to remove any impurities present like rust, dust or greasy surface. Iron nails are rubbed with sandpaper so as to remove any impurities present like rust, dust or greasy surface.

Does the colour of the copper sulphate solution change?

Yes, the colour of the copper sulphate solution changes from blue to light greenish.

What does the greenish colour of the solution show?

The greenish colour of the solution shows that Fe 2+ Ions are present in the solution.

What does the brown coating on the iron nails show?

The brown coating in the iron nail shows that copper is deposited in it by displacing iron.

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Rusting of Iron: Introduction, Chemical Reaction

Rusting of Iron: We all must have come across some rusty material or iron while wandering outside. The reddish colour on the metal is called  rusting of iron . When iron metal is exposed to air for a long time, it oxidises and forms a reddish-brown colour iron oxide on its surface. This red-brown substance is known as rust, and the process of forming rust is known as rusting.The iron rusting formula is  4Fe + 3O2 + 6H2O → 4Fe(OH)3.  Activities such as interaction with less-active metals, acids, iron stresses, and the presence of rust itself frequently speed up the process.

In this article we have provided detailed information on rusting of iron, rusting of iron is an example, rusting process, rusting of iron reaction etc. continue reading this article to get more information on this and make no mistakes while answering questions related to rusting of iron.

Rusting of Iron: Overview

Rusting is the phenomenon of the deposition of a reddish-brown coating on the surface of iron by the action of moist air, and the reddish-brown coating is known as rust. In simple words, when an iron object is left in damp air for a considerable time, it gets covered with a red-brown flaky substance called rust. This phenomenon is called rusting.

The most common example of metallic corrosion is rusting of iron and steel. Many well-known examples include the rusting of exhaust systems and car bodies, water pipes, and various types of structural steelwork.

Iron rusts due to the combined action of air and water on iron. Rusting does not occur in completely dry air or pure air of water. The precise composition of the rust is determined by atmospheric conditions and the relative contributions of the factors that govern rusting. It is primarily composed of hydrated ferric oxide, so the chemical formula of rust is ({\rm{F}}{{\rm{e}}_2}{{\rm{O}}_3}{\rm{.x}}{{\rm{H}}_2}{\rm{O}}). The following reaction can roughly describe its formation:

In the presence of moist air, the outer surface of iron rusts first, and a layer of hydrated ferric oxide (rust) is deposited on the surface. This layer is soft and porous, and it may fall off if it becomes too thick. This exposes the lower layers of iron to the environment, causing them to rust. The process continues, and iron gradually loses strength.

Rusting of Iron: Rusting process

Rusting of iron is an oxidation reaction. During rusting of iron, the iron metal reacts with oxygen in the air in the presence of water to form hydrated iron \(\left( {{\rm{III}}} \right)\) oxide, \({\rm{F}}{{\rm{e}}_2}{{\rm{O}}_3}{\rm{.x}}{{\rm{H}}_2}{\rm{O}}\).

Rust is the name given to this hydrated iron (Ill) oxide. As a result, rust is primarily hydrated iron \(\left( {{\rm{III}}} \right)\) oxide, \({\rm{F}}{{\rm{e}}_2}{{\rm{O}}_3}{\rm{.x}}{{\rm{H}}_2}{\rm{O}}\). Rust is a reddish-brown colour. We have all seen red-brown rust on iron nails, screws, pipes, and railings here and there. Not only does iron rust, but steel rusts as well when exposed to damp air. Steel, on the other hand, rusts less easily than iron.

Rusting of Iron is a Chemical Change

Rust is iron oxide \(\left( {{\rm{F}}{{\rm{e}}_2}{{\rm{O}}_3}} \right)\). Rust is something which is deposited on iron and they are not the same. Rusting of iron is a chemical change because a new substance called ‘iron oxide’ is formed during this process.

The Conditions Necessary for Rusting of Iron

Both oxygen and water must be present for the rusting of iron to occur. So, the rusting of iron is caused and governed by the following factors:

• Presence of air
• Presence of moisture

Experiment to Prove that Air and Moisture are Essential for Rusting

Procedure to demonstrate that rusting requires moisture and air..

• Place clean iron nails in each of three test tubes labelled \({\rm{A}},\,{\rm{B}}\), and \({\rm{C}}.\)
• Pour some tap water into test tube \({\rm{A}}\) and cork it.
• Pour boiled distilled water into test tube \({\rm{B}}\), then add about \(1\,{\rm{ml}}\) of oil and cork it. The oil will float on the water, preventing the air from dissolving.
• Place some anhydrous calcium chloride in test tube \({\rm{C}}\) and cork it. If there is any moisture in the air, anhydrous calcium chloride will absorb it.
• Allow these test tubes to sit for a few days before observing.

Observation

It is observed that iron nails rust in test tube \({\rm{a}}\) but not in test tubes \({\rm{b}}\) and \({\rm{C}}\). Because the nails in test tube \({\rm{a}}\) are exposed to both air and water, therefore, the nails become rusted. The nails in test tube \({\rm{b}}\) are only exposed to water, while the nails in test tube \({\rm{C}}\) are exposed to dry air.

This experiment shows that both air (oxygen) and moisture are essential for rusting to take place.

Rusting Damages Iron Objects

Rust is soft and porous, and it slowly falls off the surface of a rusted iron object, causing the iron beneath to rust. Thus, iron rusting is a continuous process that slowly eats away at iron objects, making them useless. Because iron is used to make a wide range of objects and articles, such as bridges, grills, railings, gates, and the bodies of cars, buses, trucks, and ships, rusting of iron causes significant loss over time. It is self-evident that we should have some means of preventing iron from rusting.

How do we Prevent Rusting of Iron?

The wasting of iron objects due to rusting causes a significant loss to the country’s economy and must be avoided. Several methods are used to protect iron objects from rusting. The majority of the methods involve coating the iron object with ‘something’ to keep out air and water. The following are some of the most common methods for preventing rusting of iron:

• Rusting of iron can be prevented by painting : The most common method of preventing the rusting of iron is to coat its surface with paint. When the paint is applied to the surface of an iron object, air and moisture are prevented from coming into contact with the iron object, and thus rusting does not occur. Window grills, railings, iron bridges, steel furniture, railway coaches, and the bodies of cars, buses, and trucks, among other things, are all painted regularly to keep them from rusting.
• Rusting of iron can be prevented by applying grease or oil : When some grease or oil is applied to the surface of an iron object, then air and moisture cannot come in contact with it, and hence rusting is prevented. For example, to avoid corrosion, iron and steel tools and machine parts are rubbed with grease or oil.
• Rusting of iron can be prevented by galvanisation : Articles that are exposed to extreme moisture, such as roof sheets and pipes, are protected from Rusting by galvanising. Galvanization is the process of coating steel and iron with a thin layer of zinc to prevent rusting. The iron coated with zinc is called galvanised iron. As zinc is more reactive than iron, it reacts with oxygen in the presence of moisture to form an invisible layer of zinc oxide which protects it from further Rusting. It is interesting to note that galvanised iron articles remain protected from rusting even if zinc coating is broken. This is because zinc is more reactive than iron.
• Rusting of iron can be prevented by electroplating : Another technique used to prevent articles from rusting is electroplating. Metals that do not corrode, such as tin, nickel, and chromium, are electroplated on iron in this process. This process not only prevents rusting but also improves the appearance of the articles. Some of the articles that are chromium-plated are bathroom fittings and vehicle parts such as bicycle handlebars, car bumpers, and so on.
• Rusting of iron can be prevented by alloying it to make stainless steel : When iron is alloyed with chromium and nickel, stainless steel is formed. Stainless steel does not rust at all. Cooking utensils, scissors, surgical instruments, etc., are made of stainless steel and do not rust at all. However, stainless steel is too expensive to be used in large quantities.
• Rusting of iron can be prevented by tinning : Tin is non-toxic and has a lower reactivity than iron. Food cans are tinned, which means they are thinly coated with tin. So, when a thin layer of tin metal is deposited on iron and steel objects by electroplating, then the iron and steel objects are protected from rusting. Tin-plated tiffin boxes are used because they are non-poisonous and do not contaminate the food stored inside.
• Rusting of iron can be prevented by Enameling : Enameling is a process by which powdered glass is fused to a metal substrate at high heat. Enamels can be applied to glass-ceramics.

Rusting of Iron: Summary

Rusting of iron is the deposition of a reddish-brown coating on the surface of iron by the action of moist air. This reddish-brown coating is known as rust and is called hydrated iron \(\left( {{\rm{III}}} \right)\) oxide, \({\rm{F}}{{\rm{e}}_2}{{\rm{O}}_3}{\rm{.x}}{{\rm{H}}_2}{\rm{O}}.\) The condition necessary for rusting of iron is the presence of air and presence of moisture. Rusting of iron can be prevented by applying a coating of paint, grease and oil, galvanisation, etc.

FAQs on Rusting of Iron:

Here are some of the frequently asked questions on Rusting or Iron:

Q.1. What is the process of rusting of iron? Ans: Rusting of iron is an oxidation reaction. During iron rusting, the iron metal reacts with oxygen in the air in the presence of water to form hydrated iron \(\left( {{\rm{III}}} \right)\) oxide, \({\rm{F}}{{\rm{e}}_2}{{\rm{O}}_3}{\rm{.x}}{{\rm{H}}_2}{\rm{O}}.\) Rust is the name given to this hydrated iron \(\left( {{\rm{III}}} \right)\) oxide. As a result, rust is primarily hydrated iron \(\left( {{\rm{III}}} \right)\) oxide, \({\rm{F}}{{\rm{e}}_2}{{\rm{O}}_3}{\rm{.x}}{{\rm{H}}_2}{\rm{O}}.\) Rust is a red-brown colour.

Q.2. What is rusting of iron called? Ans: Rusting is the phenomenon of the deposition of a reddish-brown coating on the surface of iron by the action of moist air, and the reddish-brown coating is known as rust.

Q.3. What is rust? Give the equation for the formation of rust? Ans: When iron metal is exposed to air for a long time, it gets oxidises and forms a reddish-brown colour iron oxide on its surface. This red-brown substance is known as rust. The equation for the formation of rust is;

Q.4. What is rusting of iron with example? Ans: Rusting is the phenomenon of the deposition of a reddish-brown coating on the surface of iron by the action of moist air, and the reddish-brown coating is known as rust. Examples:

Many well-known examples include the rusting of exhaust systems and car bodies, water pipes, and various types of structural steelwork.

Q.5. How rusting of iron can be prevented? Ans: Rusting of iron can be prevented by a. applying paint b. applying grease or oil c. by galvanisation d. by electroplating e. by alloying iron to make stainless steel f. by tinning g. by Enameling

Study About Oxidation and Reduction

We hope this article on ‘Rusting of Iron’ has helped you. If you have any queries related to rusting of iron is an example of which type of reaction? whether rusting of iron a chemical change or not? what is rusting of iron reaction? or some other query please feel to drop a comment below and we will get back to you .

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Rusting of Iron – Explanation, Chemical Reaction, Prevention

Rusting of Iron is the process by which the Rust is produced. Rust in Chemistry is a chemical compound that is formed by the Oxidation of Iron and it is reddish brown in color. Rust is formed when Iron reacts with water in the presence of water.

Rusting of iron is very harmful to various machines and other equipment that are made of Iron, as it makes them weak and decreases the life of the machine. In this article, we will learn about the Rusting of Iron, Factors affecting the Rusting of Iron, and others in detail.

Table of Content

Rusting of Iron

What is chemistry behind the rusting of iron, factors affecting the rusting of iron, what are damages caused by rusting of iron objects, how can rusting be prevented, why is rusting an undesirable phenomenon.

Rusting is the phenomenon of a reddish-brown coating forming on the surface of iron due to the action of wet air, and the reddish-brown coating is referred to as rust. Simply said, rust is a red-brown flaky substance that forms when an iron object is exposed to wet air for an extended period of time. Rusting is the term for this phenomenon. Rusting is oxidation of iron.

Rusting of iron and steel is the most prevalent example of metallic corrosion . Rusting of exhaust systems and vehicle bodywork, water pipes, and many sorts of structural steelwork are all well-known instances. The combined action of air and water on iron causes it to rust. Rusting does not happen in fully dry air or in the air that is completely devoid of water. Atmospheric conditions and the relative contributions of the components that regulate rusting define the particular composition of the rust. It is primarily composed of hydrated ferric oxide, so the chemical formula of rust is Fe 2 O 3 .xH 2 O .The following response can roughly characterize its formation:

4Fe + 3O 2 +2xH 2 O → 2Fe 2 O 3 .xH 2 O

The outer surface of iron rusts first in the presence of wet air, and a layer of hydrated ferric oxide (rust) is deposited on the surface. This layer is delicate and porous, and if it becomes too thick, it may fall off. The lowest layers of iron are exposed to the environment, causing them to rust. Iron eventually loses its strength as the process continues.

Iron rusting is an oxidation reaction. During rusting, iron combines with oxygen in the air in the presence of water to generate Fe 2 O 3 .xH 2 O, a hydrated iron (III) oxide.

This hydrated iron (Ill) oxide is referred to as rust. Rust is largely hydrated Iron (III) Oxide, Fe 2 O 3 .xH 2 O . The color of rust is reddish-brown. We’ve all noticed reddish-brown rust on iron nails, screws, pipes, and railings. When exposed to wet air, not just iron, but also steel, rusts. Steel, on the other hand, is more resistant to rust than iron.

Rusting of Iron is a Chemical Change

Rust is formed when iron (or an alloy of iron) is exposed to oxygen in the presence of moisture. This reaction is not instantaneous; rather, it takes place over a long period of time. Iron oxides are formed when oxygen atoms combine with iron atoms. The bonds between the iron atoms in the object/structure are weakened as a result.

The oxidation state of iron increases as a result of the rusting reaction, which is followed by the loss of electrons. Rust is primarily composed of two types of iron oxides that differ in the oxidation state of the iron atom. These are the oxides:

• Iron (II) oxide is also known as Ferrous Oxide. This substance has an oxidation state of +2 and the chemical formula FeO .
• Iron(III) oxide, often known as Ferric Oxide, is a compound in which the iron atom has an oxidation state of +3. Fe 2 O 3 is the chemical formula for this substance.

Iron is a reducing agent, but oxygen is an excellent oxidizing agent. When exposed to oxygen, the iron atom easily gives away electrons. The chemical reaction is described as follows:

Fe → Fe 2+ + 2e –

When water is present, the oxygen atom increases the oxidation state of iron.

4Fe 2+ + O 2 → 4Fe 3+ + 2O 2-

The iron cations and water molecules now undergo the following acid-base reactions.

Fe 2+ + 2H 2 O ⇌ Fe(OH) 2 + 2H + Fe 3+ + 3H 2 O ⇌ Fe(OH) 3 + 3H +

The direct reaction between the iron cations and the hydroxide ions also produces iron hydroxides.

O 2 + H 2 O + 4e – → 4OH – Fe 2+ + 2OH – → Fe(OH) 2 Fe 3+ + 3OH – → Fe(OH) 3

The iron hydroxides that result are now dehydrated, yielding the iron oxides that makeup rust. Many chemical processes are involved in this process, some of which are given below.

Fe(OH) 2 ⇌ FeO + H 2 O 4Fe(OH) 2 + O 2 + xH 2 O → 2Fe 2 O 3 .(x+4)H 2 O Fe(OH) 3 ⇌ FeO(OH) + H 2 O FeO(OH) ⇌ Fe 2 O 3 + H 2 O

All of the chemical reactions listed above have one thing in common: they all require the presence of water and oxygen. As a result, the amount of oxygen and water surrounding the metal can be limited to prevent rusting.

Many factors contribute to the rusting of iron, including the amount of moisture in the air and the pH of the surrounding environment. The following are a few of these elements.

• Moisture: The availability of water in the environment limits the corrosion of iron. The most prevalent cause of rusting is exposure to rain.
• The rusting process is accelerated if the pH of the environment around the metal is low. When iron is exposed to acid rain, it rusts more quickly. Iron corrosion is slowed by a higher pH.
• Due to the presence of various salts in the water, iron rusts more quickly. Many ions in saltwater speed up the rusting process through electrochemical processes.
• Impurity: When compared to iron having a variety of metals, pure iron rusts more slowly.

The size of the iron object can also influence how quickly it rusts. A huge iron object, for example, is likely to have minor flaws due to the smelting process. These flaws provide a platform for environmental attacks on the metal.

Experiment to Prove that Air and Moisture are Essential for Rusting

Procedure to demonstrate that rusting requires moisture and air.

• Clean iron nails should be placed in each of the three test jars labelled A, B, and C.
• Fill test tube A with tap water and cork it.
• Fill test tube B with hot distilled water, then add roughly 1ml of oil and cork it. The oil will float on the surface of the water, keeping the air from evaporating.
• Fill test tube C with anhydrous calcium chloride and cork it. Any moisture in the air will be absorbed by anhydrous calcium chloride.
• Allow a few days for these test tubes to settle before observing.

Observation

Iron nails rust in test tube A but not in test tubes B and C, according to the results. The nails in test tube A corroded because they were exposed to both air and water. Test tube B’s nails are solely exposed to water, but test tube C’s nails are exposed to dry air.

This experiment demonstrates that rusting requires both air (oxygen) and moisture to occur.

Rust is permeable and soft, and as it slips off the surface of a rusty iron object, the iron beneath rusts. As a result, iron rust is a constant process that eats away at iron items over time, rendering them worthless. Rusting of iron causes significant damage over time since it is used to build a wide range of structures and commodities, including bridges, grills, railings, gates, and the bodies of cars, buses, trucks, and ships. It goes without saying that we should have a way to keep iron from rusting.

The loss of iron objects due to rusting has a huge economic impact on the country, and it must be avoided. To keep iron things from rusting, a variety of techniques are employed. To keep air and water out, the majority of the ways require covering the iron piece with something. The following are some of the most prevalent ways to keep iron from rusting:

Rusting of Iron can be Prevented by Painting:

Coating the surface of the iron with paint is the most popular way to keep it from rusting. When the paint is placed on the surface of an iron object, it prevents air and moisture from getting into touch with the object, preventing rusting. To prevent rusting, window grills, railings, iron bridges, steel furnishings, railway coaches, and the bodies of automobiles, buses, and trucks, among other things, are all painted on a regular basis.

Rusting of Iron can be Prevented by Applying Grease or Oil:

When grease or oil is placed on the surface of an iron object, air and moisture are kept from coming into touch with it, preventing corrosion. Iron and steel tools and machine parts, for example, are rubbed with grease or oil to prevent corrosion.

Rusting of Iron can be Prevented by Alloying:

Stainless steel is created when the iron is alloyed with chromium and nickel. Stainless steel is impervious to rust. Stainless steel cooking utensils, scissors, and medical equipment, for example, do not corrode. Stainless steel, on the other hand, is too expensive to be utilized in big quantities.

Tin is non-toxic, and its reactivity is lower than that of iron. Food cans are tinned, which implies that they have a thin layer of tin on them. As a result, when an electroplated thin coating of tin metal is deposited on iron and steel items, the iron and steel objects are protected from rusting. Tin-plated tiffin boxes are utilized because they are non-toxic and do not contaminate the food within. Tinning prevents the rusting of Iron.

Enameling is a high-heat procedure that involves fusing powdered glass into a metal substrate. Enamels can be used on a variety of surfaces, including glass and ceramics. Enameling prevents the rusting of Iron.

Galvanization

Galvanizing protects articles exposed to excessive moisture, such as roof sheets and pipelines, against rusting. Galvanization is the technique of applying a thin layer of zinc to steel and iron to prevent rust. Galvanized iron is iron that has been zinc-coated. Zinc is more reactive than iron, therefore in the presence of moisture, it interacts with oxygen to generate an invisible layer of zinc oxide that protects it from further rusting. It’s worth noting that even if the zinc coating on galvanised iron products is broken, they remain rust-free. Because zinc is more reactive than iron, this is the case.

Electroplating

Electroplating is another method for keeping items from rusting. In this procedure, noncorroding metals including tin, nickel, and chromium are electroplated on iron. This technique not only keeps the goods from rusting but also improves their beauty. Bathroom fittings and vehicle elements such as bicycle handlebars, car bumpers, and so on are examples of chromium-plated items.

Rusting of iron is very undesirable phenomenon and it makes Iron very weak. It makes iron flaky and weak, and degraded its strength, appearance and permeability. Rusting of Iron can lead to damage to automobiles, railings, grills, and other iron structure. It reduces the life of the Iron product and makes them risky to use.

• Redox Reaction
• Plaster of Paris
• Caustic Soda, Washing Soda and Baking Soda

Sample Questions on Rusting of Iron

Question 1: What is the Process of Rusting Iron?

Iron rusting is an oxidation reaction. In the presence of water, the iron metal interacts with oxygen in the air to generate hydrated iron (III) oxide, Fe 2 O 3 .xH 2 O. This hydrated iron (III) oxide is referred to as rust. Rust is largely hydrated iron (III) oxide, Fe 2 O 3 .xH 2 O, as a result. Rust is a reddish-brown hue

Question 2: What is Rusting of Iron Called?

Rusting is the phenomena of a reddish-brown coating forming on the surface of iron due to the action of wet air, and the reddish-brown coating is referred to as rust.

Question 3:  How Rusting of Iron can be Prevented?

Rusting of iron can be prevented by following methods, Applying paint Applying grease or oil By Galvanization By electroplating Using alloying iron to make stainless steel By Tinning Using Enameling

Question 4: What is Rust?

When iron is exposed to air for an extended period of time, it oxidizes and develops a reddish-brown iron oxide on the surface. Rust is the name for this reddish-brown material. Rust is formed via the following equation, 4Fe + 3O 2 +2xH 2 O → 2Fe 2 O 3 .xH 2 O

Question 5: How does Rust Damage Iron Objects?

Question 6: What are the Conditions Necessary for Rusting?

Many factors contribute to the rusting of iron, including the amount of moisture in the air and the pH of the surrounding environment. The following are a few of these elements. Moisture: The availability of water in the environment limits the corrosion of iron. The rusting process is accelerated if the pH of the environment around the metal is low. Due to the presence of various salts in the water, iron rusts more quickly. Impurity: When compared to iron having a variety of metals, pure iron rusts more slowly.

Also Check,

• Chlorine (Cl)
• Strong and Weak Bases
• Important Compounds of Sodium

Rusting of Iron-FAQs

1. what are physical and chemical changes.

The changes that occurs in a compound are called changes. The changes that occurs in the physical properties of the compound are called the physical changes, whereas the changes that occurs the chemical properties of the compound are called the chemical changes.

2. Is the Rusting of Iron a Physical or Chemical change?

Rust is made up of Iron Oxide (Fe 2 O 3 ). As a result, rust and iron are not synonymous. Rust is an oxidation reaction and thus it is an chemical change.

3. What Causes Iron to Rust?

Rust is an oxidation reaction and it occurs when iron is reacted with oxygen and water.

4. What is the Chemical Reaction of Rust?

The chemical reaction of the rust is, 4Fe + 3O 2 + 6H 2 O → 4Fe(OH) 3 .

5. What Type of Chemical Reaction is the Rusting of Iron?

Rusting of Iron is an Oxidation Reaction.

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Observing Rusting Behavior of Iron Nails Exposed to Different Chemical Solutions

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This experiment aimed to investigate the rusting behavior of iron nails when exposed to different chemical solutions (HCl, NaCl, HNO3, NaOH) and open air. The study observed the time it took for observable changes to occur in each subject and documented the rusting process over a span of 7 days.

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Notable findings include variations in the rate of corrosion among different solutions and the impact of pH levels on the corrosion process. The experiment provided insights into the practical implications of rust prevention in various industrial settings.

Experiment Question

In what time can each subject's changes be fully observed? In what time can rusting occur and be fully observed for each subject?

If you drop a nail into a tube filled with different chemicals (HCl, NaCl, HNO3, NaOH) and leave a nail exposed to open air, then rusting will occur due to the chemical structure of the solutions.

Introduction

Rusting of iron nails is of significant concern, especially in industries that deal with essential and potentially hazardous objects.

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Understanding when and how iron nails rust is essential for maintenance and safety.

Rust is the common name for iron oxide (Fe2O3), which can come in various colors due to different chemical compositions. Rusting occurs when iron is exposed to oxygen or other oxidizing agents, leading to corrosion. This process involves a chemical reaction called oxidation, where iron loses electrons to oxygen.

This experiment focuses on observing the rusting of iron nails when exposed to different substances (HCl, NaCl, HNO3, NaOH) over a span of 7 days.

Literature Review

Rusting of iron and steel materials is a well-known natural phenomenon that occurs when iron is exposed to oxygen or other oxidizing agents. The process involves a chemical reaction called oxidation, where iron loses electrons to oxygen, resulting in the formation of iron oxide, commonly known as rust (Fe2O3) [1]. Rusting can lead to the corrosion and weakening of iron and steel structures, making it a significant concern in various industries, including construction, engineering, and manufacturing [2].

The rate of rusting depends on several factors, including the presence of moisture, temperature, and the chemical environment. Acids, such as hydrochloric acid (HCl) and nitric acid (HNO3), are known to accelerate the corrosion process due to their low pH levels [3]. In contrast, alkaline solutions like sodium hydroxide (NaOH) tend to have a slower effect on rusting [4]. Sodium chloride (NaCl), commonly found in saltwater, can also contribute to corrosion when iron is exposed to it [5].

Previous studies have investigated the kinetics of rust formation and the factors influencing rusting rates. These studies have utilized various methods, including electrochemical analysis, to understand the underlying mechanisms of corrosion [6]. However, the practical observation of rusting over time is essential for real-world applications, such as maintenance and material selection.

Our experiment seeks to contribute to this body of knowledge by providing practical insights into the timeframes within which observable rusting occurs in different chemical environments. By understanding when rust becomes noticeable, we can better inform maintenance and corrosion prevention strategies in industries where iron and steel are commonly used.

• The researchers wore personal protective equipment, including lab gowns and gloves.
• Laboratory equipment like test tube racks, test tubes, watch glass, nails, and sandpaper were prepared and placed on a flat surface for safety.
• Each test tube was filled with approximately 8 ml of the provided solutions.
• The iron nails were placed simultaneously inside each test tube containing different solutions and one was exposed to open air.
• The researchers observed and recorded changes in the nails over time, noting the time, day, pH level, and a description of each subject's condition.

In this experiment, changes in the subjects were not noticeable before they were submerged in the solutions. However, the most significant reactions were observed in HNO3 (Nitric acid) and HCl (Hydrochloric acid) within the first hour, although they did not rust initially. NaOH (Sodium hydroxide) and NaCl (Sodium chloride) showed hardly any changes within the first hour of exposure to their solutions.

Over 2 hours, HNO3 exhibited the most drastic changes, with a color change in the solution, darkening of the nail's surface and bottom, and the presence of bubbles. HCl produced the most bubbles from the beginning, with a solution color change after 3 hours and continuous fumes. NaCl showed a color change primarily at the bottom of the solution. NaOH had no observable changes.

After a week, the results were as follows: - HCl solution had rusted - NaOH showed no changes - HNO3 was completely covered in rust - NaCl had rust at the bottom of the solution and on the nail - The nail exposed to air began to rust

Two acid solutions, HNO3 and HCl, corroded faster due to their low pH levels. These two acids corroded quickly, as evidenced by their changes in the data. However, the researchers were interested not only in the changes but also in the rusting of the iron.

The experiment successfully answered the questions regarding the time it takes for changes to be observed in each subject and when rusting occurs. Notable findings include:

• HNO3 exhibited changes in less than 1 hour, with rusting occurring in 4 days.
• NaOH showed no changes within a week.
• HCl exhibited changes in less than 1 hour.
• NaCl showed a solution color change and some bubbles after 3 hours, with rusting in 4 days.
• The nail exposed to air began rusting within a week.

The experiment was limited by time constraints, and it is possible that NaOH could exhibit changes with more time. Nevertheless, the research successfully answered the questions and provided valuable insights into the behavior of iron nails exposed to different solutions.

In real-world scenarios, it is essential to prevent and monitor the corrosion of various materials, not just iron nails. Different materials have their weaknesses that may lead to corrosion or deterioration. In engineering, managing and protecting materials from hazards is crucial to maintain structural integrity and prevent harm to the environment.

"Some people shine first, rust first." - Iron Nail

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