Exam 19: The Kinetic Theory of Gases

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

An ideal gas of N diatomic molecules has temperature T. If the number of molecules is doubled without changing the temperature, the internal energy increases by:

The mean free path of a gas molecule is:

A 2.0-m³ weather balloon is loosely filled with helium at 1 atm (76 cm Hg) and at 27 $\degree$ C. At an elevation of 20,000 ft, the atmospheric pressure is down to 38 cm Hg and the helium has expanded, being under no constraint from the confining bag. If the temperature at this elevation is -48 $\degree$ C, the gas volume is:

When work W is done on an ideal gas of diatomic molecules in thermal isolation the increase in the total translational kinetic energy of the molecules is:

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 speeds are the same if the ratio of the temperatures T_A/T_B is:

273 cm³ of an ideal gas is at 0 $\degree$ C. It is heated at constant pressure to 10 $\degree$ C. It will now occupy:

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

Two identical rooms in a house are connected by an open doorway. The temperatures in the two rooms are maintained at different values. Which room contains more air?

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:

A certain ideal gas has a temperature 300 K and a pressure 5.0 * 10⁴ Pa. The molecules have a mean free path of 4.0 *10^-7m. If the temperature is raised to 350 K and the pressure is reduced to 1.0 * 10⁴ Pa the mean free path is then:

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

When work W is done on an ideal gas of N diatomic molecules in thermal isolation the temperature increases by:

In a certain gas the molecules are 5.0 *10^-9 m apart on average, have a mean free path of 5.0 * 10^-6 m, and have an average speed of 500 m/s. The rate at which a molecule has collision with other molecules is about:

The mean free path of molecules in a gas is:

An ideal gas has molar specific heat C_p at constant pressure. When the temperature of n moles is increased by $\Delta$ T the increase in the internal energy is:

An ideal monatomic gas has a molar specific heat C_v at constant volume of:

The difference between the molar specific heat at constant pressure and the molar specific heat at constant volume for an ideal gas is:

When work W is done on an ideal gas of diatomic molecules in thermal isolation the increase in the total rotational energy of the molecules is:

Assume that helium behaves as an ideal monatomic gas. If 2 moles of helium undergo a temperature increase of 100 K at constant pressure, how much work is done by the gas?