Exam 19: The Kinetic Theory of Gases

The diagram shows three isotherms for an ideal gas, with T₃-T₂ the same as T₂-T₁.It also shows five thermodynamic processes carried out on the gas.Rank the processes in order of the change in the internal energy of the gas, least to greatest.

Two ideal monatomic gases are in thermal equilibrium with each other.Gas A is composed of molecules with mass m while gas B is composed of molecules with mass 4m.The ratio of the average molecular speeds v_A/v_B is:

The specific heat of a polyatomic gas is greater than the specific heat of a monatomic gas because:

The energy absorbed as heat by an ideal gas for an isothermal process equals:

An isothermal process for an ideal gas is represented on a p-V diagram by:

For a given change in temperature, the change in the internal energy of an ideal gas:

TV ^$\gamma$ is constant for an ideal gas undergoing an adiabatic process, where $\gamma$ is the ratio of heat capacities C_p/C_v.This is a direct consequence of:

In an adiabatic expansion,

The heat capacity at constant volume and the heat capacity at constant pressure have different values because:

The pressure of an ideal gas of diatomic molecules is doubled by halving the volume.The ratio of the new internal energy to the old, both measured relative to the internal energy at 0 K, is:

During a slow adiabatic expansion of a gas:

The pressure of an ideal gas is doubled during a process in which the energy given up as heat by the gas equals the work done on the gas.As a result, the volume is:

As the volume of an ideal gas is increased at constant pressure the average molecular speed:

During a reversible adiabatic expansion of an ideal gas, which of the following is NOT true?

Ideal monatomic gas A is composed of molecules with mass m while ideal monatomic gas B is composed of molecules with mass 4m.The average molecular energies are the same if the ratio of the temperatures T_A/T_B is:

A real gas undergoes a process which can be represented as a curve on a p-V diagram.This curve is an isotherm if:

Oxygen (molar mass = 32 g)occupies a volume of 12 liters when its temperature is 20°C and its pressure is 1 atm.Using R = 0.082 liter.atm/mole.K, calculate the mass of the oxygen:

If the temperature T of an ideal gas is increased at constant pressure the mean free path:

In using the ideal gas law, the temperature T must be measured in:

Air enters a hot-air furnace at 7°C and leaves at 77°C.If the pressure does not change each entering cubic meter of air expands to: