GCSE Physics GCSE Biology GCSE Chemistry GCSE Mathematics
Related Topics
- Absolute zero and the Kelvin scale of temperature
- Pressure and volume relationship of a gas – Boyle's law
- Volume and temperature relationship of a gas – Charles' law
- Pressure and temperature relationship of a gas – the Pressure Law
- The gas equation
Volume and temperature relationship of a gas
Charles' law.
The relationship between the volume and temperature of a gas was first put forward by the French scientist Jacques-Alexandre-César Charles at around 1787 and is known as Charles’ Law.
Charles’ law states :
| Volume | = constant |
| Temperature |
The animation below gives and explanation of Charles' law:
A sealed cylinder with no leaks contains a fixed mass. In order to keep the gas pressure constant the piston is allowed to move freely so that the internal pressure created by the gas particles can equal the constant external pressure. If the internal pressure increases the piston will move up to allow the pressure to equalise.
The above set up is used to investigate the relationship between temperature and volume for a gas. Heat energy is applied to the cylinder and the temperature of the gas increases. The average velocity of the gas particles increases resulting in an increase in the rate of collisions and the average force per collision. This produces an increase in pressure inside the cylinder, the cylinder pressure becomes greater than the external pressure and the piston moves up increasing the volume.
By plotting the recorded values of volume (V) against temperature (T) a straight line is produced. We can see from the values that the gas expands uniformly with temperature. We can extrapolate the straight line and see the relationship between cooling the gas and the volume. Further extrapolation gives the temperature at which the volume of gas would become zero. This temperature is at -273°C and is called the absolute zero of temperature.
Converting the recorded temperatures into the Kelvin scale and plotting the volume (V) against the absolute temperature (T) gives a straight line which when extrapolated passes through the origin. This shows the volume of the gas is directly proportional to the absolute temperature of the gas. Doubling the temperature will double the volume. The gradient of the slope is the constant in Charles’ Law.
Charles’ Law Example:
Using the example of the sealed cylinder above, the volume of gas at the start is recorded as 30 cm 3 with a temperature of 30°C. The cylinder is heated further till the thermometer records 60°C. What is the volume of gas?
V/T = constant
V 1 /T 1 = V 2 /T 2 V1 = 30 cm 3 T1 = 30°C = 30+273 = 303K (remember to convert from Celsius to Kelvin) T2 = 60°C = 60+273 = 333K V2 = ? V 1 /T 1 = V 2 /T 2 V 2 = V 1 x T 2 T 1 V 2 = 30 x 333 303 = 32.97 cm 3
Boyle's Law & Charles' Law
Investigation of boyle's law.
Boyle’s Law describes the relationship between the pressure and volume of a fixed mass of gas at constant temperature.
Manometer method
- Use a pump to change the air pressure on one side of the manometer.
- Use a pressure gauge on the pump side to measure air pressure, which is equal to the pressure of the air in the glass tube.
- You can measure the volume of trapped air.
- Record the volume for several different pressure values.
Analysis of manometer method
- If you plot a graph of volume against pressure, you get a monotonically decreasing curve.
- Plot a graph of V -1 against P and the best fit straight line goes through the origin.
- This verifies that V -1 is directly proportional to the pressure, i.e. pV is a constant or that P and V are inversely proportional to each other. This assumes that the temperature and mass of the gas is constant.
Further analysis of manometer method
- Plot log(V) against log (P). It doesn’t matter what base logarithm you use.
- The gradient of the line of best fit should be -1.
- log(V) = log(k) - log(P).
- log(V) = - log(P) + log(k).
Further analysis of manometer method 2
- Compare the last line with y = mx + c.
- If log(V) is plotted on the y-axis, with log(P) on the x-axis, the gradient = -1 and the y-intercept should be log(k).
- You can find the constant, k, using k = Z c , where Z is the base of the logarithms (i.e. 10 or e) and c is the y-intercept.
Investigation of Boyle's Law 2
Syringe and data logging method
- Connect the open end of a syringe to a pressure sensor (which is then connected to data logger and computer).
- Start recording on data logger.
- Move the plunger in steps, i.e. decrease or increase the volume of trapped gas slowly so as not to warm or cool the gas.
- For each new volume, record the pressure.
Syringe and data logging method 2
- Use software, such as a spreadsheet, to plot a graph of volume against pressure to get a monotonically decreasing curve.
- Use software to plot a graph of V -1 against P.
- i.e. PV = constant or that P and V are inversely proportional to each other, assuming that the temperature and mass of the gas is constant.
Investigation of Charles’ Law
Charles’ Law describes the relationship between the volume and absolute temperature of a fixed mass of gas at constant pressure.
- Set up the apparatus as shown in the diagram.
- Caution: it is common practice to use a kerosene-based oil, which needed a separate risk assessment because it is available via CLEAPPS.
- Keep stirring the water so as to reduce temperature gradients through the water.
- The length of the air column is directly proportional to the volume of trapped air. This assumes that the inner diameter of the capillary tube is constant.
- I.e. extended back to -400 °C so that an extrapolation back to the temperature axis can give a value for absolute zero.
- Notice that the values of volume and temperature are all bunched to the right.
- The extrapolation is suspect because you have to extrapolate a long way before the line hits the temperature axis.
- Repeating this with different gases, different volumes of gas and at different pressures gives different straight lines. All of the best fit straight lines should pass through the same point on the temperature axis.
Plot the graph again
- If you plot the graph again using the student’s value for absolute zero, the length-temperature graph becomes a straight line through the origin as shown.
- This shows that the volume of gas is directly proportional to the temperature in Kelvin. This assumes that the pressure and mass of the gas are constant.
1 Measurements & Errors
1.1 Measurements & Errors
1.1.1 Use of SI Units
1.1.2 SI Prefixes, Standard Form & Converting Units
1.1.3 End of Topic Test - Units & Prefixes
1.1.4 Limitation of Physical Measurements
1.1.5 Uncertainty
1.1.6 Estimation
1.1.7 End of Topic Test - Measurements & Errors
2 Particles & Radiation
2.1 Particles
2.1.1 Atomic Model
2.1.2 Specific Charge, Protons & Neutron Numbers
2.1.3 End of Topic Test - Atomic Model
2.1.4 Isotopes
2.1.5 Stable & Unstable Nuclei
2.1.6 End of Topic Test - Isotopes & Nuclei
2.1.7 A-A* (AO3/4) - Stable & Unstable Nuclei
2.1.8 Particles, Antiparticles & Photons
2.1.9 Particle Interactions
2.1.10 Classification of Particles
2.1.11 End of Topic Test - Particles & Interactions
2.1.12 Quarks & Antiquarks
2.1.13 Application of Conservation Laws
2.1.14 End of Topic Test - Leptons & Quarks
2.1.15 Exam-Style Question - Radioactive Decay
2.2 Electromagnetic Radiation & Quantum Phenomena
2.2.1 The Photoelectric Effect
2.2.2 The Photoelectric Effect Explanation
2.2.3 End of Topic Test - The Photoelectric Effect
2.2.4 Collisions of Electrons with Atoms
2.2.5 Energy Levels & Photon Emission
2.2.6 Wave-Particle Duality
2.2.7 End of Topic Test - Absorption & Emission
3.1 Progressive & Stationary Waves
3.1.1 Progressive Waves
3.1.2 Wave Speed & Phase Difference
3.1.3 Longitudinal & Transverse Waves
3.1.4 End of Topic Test - Progressive Waves
3.1.5 Polarisation
3.1.6 Stationary Waves
3.1.7 Stationary Waves 2
3.1.8 End of Topic Test - Polarisation & Stationary Wave
3.1.9 A-A* (AO3/4) - Stationary Waves
3.2 Refraction, Diffraction & Interference
3.2.1 Interference
3.2.2 Interference 2
3.2.3 End of Topic Test - Interference
3.2.4 Diffraction
3.2.5 Diffraction Gratings
3.2.6 End of Topic Test - Diffraction
3.2.7 Refraction at a Plane Surface
3.2.8 Internal Reflection & Fibre Optics
3.2.9 End of Topic Test - Refraction
3.2.10 Exam-Style Question - Waves
4 Mechanics & Materials
4.1 Force, Energy & Momentum
4.1.1 Scalars & Vectors
4.1.2 Vector Problems
4.1.3 End of Topic Test - Scalars & Vectors
4.1.4 Moments
4.1.5 Centre of Mass
4.1.6 End of Topic Test - Moments & Centre of Mass
4.1.7 Motion in a Straight Line
4.1.8 Graphs of Motion
4.1.9 Bouncing Ball Example
4.1.10 End of Topic Test - Motion in a Straight Line
4.1.11 Acceleration Due to Gravity
4.1.12 Projectile Motion
4.1.13 Friction
4.1.14 Terminal Speed
4.1.15 End of Topic Test - Acceleration Due to Gravity
4.1.16 Newton's Laws
4.1.17 Momentum
4.1.18 Momentum 2
4.1.19 End of Topic Test - Newton's Laws & Momentum
4.1.20 A-A* (AO3/4) - Newton's Third Law
4.1.21 Work & Energy
4.1.22 Power & Efficiency
4.1.23 Conservation of Energy
4.1.24 End of Topic Test - Work, Energy & Power
4.1.25 Exam-Style Question - Forces
4.2 Materials
4.2.1 Density
4.2.2 Bulk Properties of Solids
4.2.3 Energy in Materials
4.2.4 Young Modulus
4.2.5 End of Topic Test - Materials
5 Electricity
5.1 Current Electricity
5.1.1 Basics of Electricity
5.1.2 Current-Voltage Characteristics
5.1.3 End of Topic Test - Basics of Electricity
5.1.4 Resistivity
5.1.5 Superconductivity
5.1.6 A-A* (AO3/4) - Superconductivity
5.1.7 End of Topic Test - Resistivity & Superconductors
5.1.8 Circuits
5.1.9 Power and Conservation
5.1.10 Potential Divider
5.1.11 Emf & Internal Resistance
5.1.12 End of Topic Test - Power & Potential
5.1.13 Exam-Style Question - Resistance
6 Further Mechanics & Thermal Physics (A2 only)
6.1 Periodic Motion (A2 only)
6.1.1 Circular Motion
6.1.2 Circular Motion 2
6.1.3 End of Topic Test - Circular Motion
6.1.4 Simple Harmonic Motion
6.1.5 Simple Harmonic Systems
6.1.6 Energy in Simple Harmonic Motion
6.1.7 Resonance
6.1.8 End of Topic Test - Simple Harmonic Motion
6.1.9 A-A* (AO3/4) - Simple Harmonic Motion
6.2 Thermal Physics (A2 only)
6.2.1 Thermal Energy Transfer
6.2.2 Thermal Energy Transfer Experiments
6.2.3 Ideal Gases
6.2.4 Ideal Gases 2
6.2.5 Boyle's Law & Charles' Law
6.2.6 Molecular Kinetic Theory Model
6.2.7 Molecular Kinetic Theory Model 2
6.2.8 End of Topic Test - Thermal Energy & Ideal Gases
6.2.9 Exam-Style Question - Ideal Gases
7 Fields & Their Consequences (A2 only)
7.1 Fields (A2 only)
7.1.1 Fields
7.2 Gravitational Fields (A2 only)
7.2.1 Newton's Law
7.2.2 Gravitational Field Strength
7.2.3 Gravitational Potential
7.2.4 Orbits of Planets & Satellites
7.2.5 Escape Velocity & Synchronous Orbits
7.2.6 End of Topic Test - Gravitational Fields
7.3 Electric Fields (A2 only)
7.3.1 Coulomb's Law
7.3.2 Electric Field Strength
7.3.3 Electric Field Strength 2
7.3.4 Electric Potential
7.3.5 End of Topic Test - Electric Fields
7.3.6 A-A* (AO3/4) - Electric and Gravitational Field
7.4 Capacitance (A2 only)
7.4.1 Capacitance
7.4.2 Parallel Plate Capacitor
7.4.3 Energy Stored by a Capacitor
7.4.4 Capacitor Discharge
7.4.5 Capacitor Charge
7.5 Magnetic Fields (A2 only)
7.5.1 Magnetic Flux Density
7.5.2 End of Topic Test - Capacitance & Flux Density
7.5.3 Moving Charges in a Magnetic Field
7.5.4 Magnetic Flux & Flux Linkage
7.5.5 Electromagnetic Induction
7.5.6 Electromagnetic Induction 2
7.5.7 Alternating Currents
7.5.8 Operation of a Transformer
7.5.9 Magnetic Flux Density
7.5.10 End of Topic Test - Electromagnetic Induction
8 Nuclear Physics (A2 only)
8.1 Radioactivity (A2 only)
8.1.1 Rutherford Scattering
8.1.2 Alpha & Beta Radiation
8.1.3 Gamma Radiation
8.1.4 Radioactive Decay
8.1.5 Half Life
8.1.6 End of Topic Test - Radioactivity
8.1.7 Nuclear Instability
8.1.8 Nuclear Radius
8.1.9 Mass & Energy
8.1.10 Binding Energy
8.1.11 Induced Fission
8.1.12 Safety Aspects of Nuclear Reactors
8.1.13 End of Topic Test - Nuclear Physics
8.1.14 A-A* (AO3/4) - Nuclear Fusion
9 Option: Astrophysics (A2 only)
9.1 Telescopes (A2 only)
9.1.1 Astronomical Telescopes
9.1.2 Reflecting Telescopes
9.1.3 Single Dish Radio Telescopes
9.1.4 Large Diameter Telescopes
9.2 Classification of Stars (A2 only)
9.2.1 Classification by Luminosity
9.2.2 Absolute Magnitude
9.2.3 Black Body Radiation
9.2.4 Stellar Spectral Classes
9.2.5 Hertzsprung-Russell Diagrams
9.2.6 Astronomical Objects
9.3 Cosmology (A2 only)
9.3.1 Doppler Effect
9.3.2 Hubble's Law
9.3.3 Quasars
9.3.4 Detecting Exoplanets
10 Option: Medical Physics (A2 only)
10.1 Physics of the Eye (A2 only)
10.1.1 Physics of Vision
10.1.2 Defects of Vision
10.1.3 Lenses
10.1.4 Correcting Defects of Vision
10.2 Physics of the Ear (A2 only)
10.2.1 Structure of the Ear
10.2.2 Sensitivity of the Ear
10.2.3 Hearing Defects
10.3 Biological Measurement (A2 only)
10.3.1 Electrocardiography (ECG)
10.4 Non-Ionising Imaging (A2 only)
10.4.1 Ultrasound Imaging
10.4.2 Ultrasound Imaging 2
10.4.3 Fibre Optics & Endoscopy
10.4.4 Magnetic Resonance Scanning
10.5 X-Ray Imaging (A2 only)
10.5.1 Diagnostic X-Rays
10.5.2 X-Ray Image Processing
10.5.3 Absorption of X-Rays
10.5.4 CT Scanners
10.6 Radionuclide Imaging & Therapy (A2 only)
10.6.1 Imaging Techniques
10.6.2 Half Life
10.6.3 Gamma Camera
10.6.4 High Energy X-Rays
10.6.5 Radioactive Implants
10.6.6 Imaging Comparisons
11 Option: Engineering Physics (A2 only)
11.1 Rotational Dynamics (A2 only)
11.1.1 Moment of Inertia
11.1.2 Rotational Kinetic Energy
11.1.3 Rotational Motion
11.1.4 Torque & Angular Acceleration
11.1.5 Angular Momentum
11.1.6 Angular Work & Power
11.2 Thermodynamics & Engines (A2 only)
11.2.1 First Law of Thermodynamics
11.2.2 Non-Flow Processes
11.2.3 p-V Diagrams
11.2.4 Engine Cycles
11.2.5 Second Law & Engines
11.2.6 Reversed Heat Engines
12 Option: Turning Points in Physics (A2 only)
12.1 Discovery of the Electron (A2 only)
12.1.1 Cathode Rays
12.1.2 Thermionic Electron Emission
12.1.3 Electron Specific Charge
12.1.4 Millikan's Experiment
12.2 Wave-Particle Duality (A2 only)
12.2.1 Newton's & Huygen's Theories of Light
12.2.2 Electromagnetic Waves
12.2.3 Photoelectricity
12.2.4 Wave-Particle Duality
12.2.5 Electron Microscopes
12.3 Special Relativity (A2 only)
12.3.1 Michelson-Morley Experiment
12.3.2 Einstein's Theory of Special Relativity
12.3.3 Time Dilation
12.3.4 Length Contraction
12.3.5 Mass & Energy
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Ideal Gases 2
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IMAGES
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COMMENTS
Revision notes on 6.5.6 Required Practical: Investigating Gas Laws for the AQA A Level Physics syllabus, written by the Physics experts at Save My Exams.
Charles’ law states: "For a fixed mass of gas, at a constant pressure, the volume (V) is directly proportional to the absolute temperature (T)." Volume α Temperature. The animation below gives and explanation of Charles' law: A sealed cylinder with no leaks contains a fixed mass.
How would you present your results from the Charles' Law experiment? Plot a graph of length, l (m) against temperature, θ (°C) and draw a straight line of best fit. How can you interpret your results from the Charles' Law experiment?
Charles’ law Equipment: Capillary tube Sulfuric acid 2 litre beaker 2 elastic bands 30cm ruler Thermometer Kettle Method: Set up the apparatus as shown in the diagram with the open end of the capillary tube at the top and add hot water from the kettle. The hot water should cover the air sample.
Study with Quizlet and memorise flashcards containing terms like what are we doing in Charles's law?, what are the independent variables, dependent variables and the control variables in this experiment?, what is the uncertainty of a 2 litre beaker? and others.
Method: a Fix the capillary tube and thermometer to the ruler with rubber bands at each end. Measurements are easier if the end of the air column inside the tube coincides with the zero of the centimetre scale on the rule. b Put the tubes into the deep beakers with the open end free to the air. c Add water, or water and crushed ice, to the ...
Boyle's Law & Charles' Law. Test yourself. Investigation of Boyle's Law. Boyle’s Law describes the relationship between the pressure and volume of a fixed mass of gas at constant temperature. Manometer method. Use a pump to change the air pressure on one side of the manometer.
Study with Quizlet and memorize flashcards containing terms like Charles' Law Practical Aim, assumption made for Charles' Law practical, Charles's law Practical method and more.
Charles’s Law: Charles’s Law states that the volume of a gas is proportional to the temperature of the gas for a gas at constant pressure. V \propto T. V= volume in cubic metres \text { (m}^3\text {)} T= temperature in kelvin \text { (K)}
Charles' Law. Figure 1b shows that the volume of a gas is directly proportional to its thermodynamic temperature, provided that the amount of gas and the pressure remain constant. This is known as Charles’ law, and can be expressed mathematically as where T represents the absolute temperature (usually measured in Kelvins).