Lesson 3.6.2.2

3.6.2.2 Ideal gases Quiz: AQA Physics, Unit 6

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 3.6.2.2, Ideal gases: 20 multiple choice questions for the AQA Physics (7408), Unit 6: Further mechanics and thermal physics (A-level only), written with Revision Ninja.

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The 20 questions

  1. Absolute zero of temperature is:

    • the temperature at which all gases become liquids
    • 0 degrees Celsius, the temperature at which water freezes
    • minus 100 degrees Celsius, the lowest temperature reached on Earth
    • 0 K, the lowest possible temperature, where molecular kinetic energy is at its minimum

  2. The ideal gas equation for n moles of gas is:

    • pV = nR / T
    • pT = nRV
    • p / V = nRT
    • pV = nRT

  3. In the equation pV = NkT for N molecules, k is:

    • the Boltzmann constant
    • the gas constant per mole
    • the Avogadro constant
    • the molar gas constant

  4. The Boltzmann constant is related to the molar gas constant R and Avogadro constant N_A by:

    • k = R N_A
    • k = R / N_A
    • k = N_A / R
    • k = R^2 / N_A

  5. The work done by a gas expanding at constant pressure is:

    • W = p delta T
    • W = p delta V
    • W = p / delta V
    • W = nRT

  6. The molar mass of a gas is:

    • the mass of one molecule of the gas
    • the volume occupied by one mole
    • the mass of one mole of the gas
    • the mass of Avogadro's number of moles

  7. Boyle's law states that at constant temperature:

    • pressure is inversely proportional to volume
    • pressure and volume are independent
    • pressure is directly proportional to volume
    • volume is proportional to the square of pressure

  8. Charles's law states that at constant pressure:

    • volume is directly proportional to thermodynamic (kelvin) temperature
    • volume is proportional to temperature in degrees Celsius
    • volume is inversely proportional to temperature
    • volume is independent of temperature

  9. 2.0 mol of ideal gas at 300 K occupies 0.050 m^3. What is its pressure?

    • about 1.0 x 10^3 Pa
    • about 1.0 x 10^5 Pa
    • about 4.0 x 10^5 Pa
    • about 2.5 x 10^4 Pa

  10. At 273 K and 1.01 x 10^5 Pa, what volume does 1.0 mol of ideal gas occupy?

    • about 2.2 x 10^-3 m^3
    • about 0.0022 m^3
    • about 0.022 m^3
    • about 0.22 m^3

  11. A sample contains 0.50 mol of gas. How many molecules does it contain? Take N_A = 6.0 x 10^23 mol^-1.

    • 1.2 x 10^24
    • 6.0 x 10^22
    • 3.0 x 10^23
    • 6.0 x 10^23

  12. A gas expands at constant pressure 2.0 x 10^5 Pa from 1.0 x 10^-3 m^3 to 3.0 x 10^-3 m^3. What work does it do?

    • 600 J
    • 800 J
    • 400 J
    • 200 J

  13. What is the average translational kinetic energy per molecule of an ideal gas at 300 K? Take k = 1.38 x 10^-23 J K^-1.

    • 1.0 x 10^-21 J
    • 6.2 x 10^-21 J
    • 4.1 x 10^-21 J
    • 2.1 x 10^-20 J

  14. A temperature of 27 degrees Celsius is equal to:

    • 300 K
    • 246 K
    • 27 K
    • 273 K

  15. In a Boyle's law experiment, which graph gives a straight line through the origin?

    • pressure against volume squared
    • pV against volume
    • pressure against 1/volume
    • pressure against volume

  16. The pressure of a fixed mass of gas in a sealed container is doubled at constant volume. Its absolute temperature:

    • quadruples
    • is unchanged
    • doubles
    • halves

  17. A gas at 2.0 x 10^5 Pa occupies 0.010 m^3 at constant temperature. It is compressed to 0.0050 m^3. What is the new pressure?

    • 1.0 x 10^5 Pa
    • 2.0 x 10^5 Pa
    • 8.0 x 10^5 Pa
    • 4.0 x 10^5 Pa

  18. 3.0 mol of ideal gas at 400 K occupies 0.040 m^3. What is its pressure?

    • about 2.5 x 10^4 Pa
    • about 2.5 x 10^5 Pa
    • about 1.0 x 10^5 Pa
    • about 5.0 x 10^5 Pa

  19. A student says the ideal gas law holds exactly for real gases at very high pressure and very low temperature. Which response is best?

    • Incorrect, because ideal gases contain no molecules, so the law cannot apply to any gas.
    • Correct: real gases always behave as ideal gases.
    • Correct: the ideal gas law applies to real gases at all temperatures.
    • Incorrect: at high pressure and low temperature, molecular volume and intermolecular forces become significant, so real gases deviate.

  20. Two gases in identical containers at the same temperature and pressure contain the same number of molecules. Which statement justifies this?

    • pV = mRT, so mass is fixed by the container
    • they have the same molar mass by definition
    • equal pressure means equal density for any two gases
    • pV = NkT, so N depends only on p, V and T

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