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Kinetic Theory

Molecular speeds, temperature and real gases

  • 3 things to know
  • A2 Unit 3

Overview

Recall questions on Molecular speeds, temperature and real gases.

What you need to know

Answer each one before you reveal it.

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Key term

State the equation for the total internal energy of an ideal monatomic gas in terms of n, R, and T.

Key term

Define mean square speed for gas particles.

Key term

In the equation pV = ⅓Nm(c̄²), what does N represent?

Questions from this subtopic

Each one with the model answer underneath.

  1. 1

    Define mean square speed for gas particles.

    Model answer

    The mean square speed is the average of the squares of the speeds of all particles in a gas.

  2. 2

    What is the root mean square (r.m.s.) speed of gas particles?

    Model answer

    It is the square root of the mean square speed.

  3. 3

    State the equation that relates pressure, volume, number of molecules, particle mass, and mean square speed.

    Model answer

    pV = ⅓Nm⟨c²⟩, where p is pressure, V is volume, N is the number of molecules, m is the mass of one particle, and ⟨c²⟩ is the mean square speed.

  4. 4

    In the equation pV = ⅓Nm(c̄²), what does N represent?

    Model answer

    N represents the total number of gas molecules.

  5. 5

    State the equation for the average kinetic energy of a gas particle in terms of the Boltzmann constant and temperature.

    Model answer

    Average kinetic energy = (3/2)k_B T, where k_B is the Boltzmann constant and T is the absolute temperature.

  6. 6

    What physical quantities does the Boltzmann constant relate?

    Model answer

    It relates the average kinetic energy of particles to the absolute temperature.

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