Exam 19: The Kinetic Theory of Gases

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

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:

The specific heat at constant volume of an ideal gas depends on:

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

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

A 2-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 (in m³) is:

According to the Maxwellian speed distribution, as the temperature increases the average speed:

The heat capacity at constant volume of an ideal gas depends on:

The average speed of air molecules at room temperature is about:

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:

Monatomic, diatomic, and polyatomic ideal gases each undergo slow adiabatic expansions from the same initial volume and the same initial pressure to the same final volume. The magnitude of the work done by the environment on the gas:

The pressures p and volumes V of the five ideal gases,with the same number of molecules, are given below. Which has the highest theperatures?

A sample of an ideal gas is compressed by a piston from 10 m³ to 5 m³ and simultaneously cooled from 273 $\degree$ C to 0 $\degree$ C. As a result there is:

The temperature of n moles of an ideal monatomic gas is increased by $\Delta$ T at constant volume. The energy Q absorbed as heat, change $\Delta$ E_int in internal energy, and work W done by the environment are given by:

The mean free path of air molecules at room temperature and atmospheric pressure is about:

A sample of argon gas (molar mass 40 g) is at four times the absolute temperature of a sample of hydrogen gas (molar mass 2 g). The ratio of the rms speed of the argon molecules to that of the hydrogen is:

An air bubble doubles in volume as it rises from the bottom of a lake (1000 kg/m³). Ignoring any temperature changes, the depth of the lake is:

A given mass of gas is enclosed in a suitable container so that it may be maintained at constant volume. Under these conditions, there can be no change is what property of the gas?

In a system of N gas molecules, the individual speeds are v₁, v₂, ..., v_N. The rms speed of these molecules is:

The temperature of n moles of an ideal monatomic gas is increased by $\Delta$ T at constant pressure. The energy Q absorbed as heat, change $\Delta$ E_int in internal energy, and work W done by the environment are given by: