Kinetic Theory

According to the kinetic theory of gases, which of the following assumptions is made about the molecules of an ideal gas?

The root mean square speed (v_rms) of gas molecules is given by which of the following formulas? (M = molar mass, R = gas constant, T = temperature)

Which of the following quantities is directly proportional to the average kinetic energy of the gas molecules?

In the kinetic theory, the pressure exerted by a gas on the walls of its container is due to:

Which of the following expressions correctly relates pressure (P), volume (V), and average kinetic energy (E_k) for N molecules of an ideal gas?

If the temperature of an ideal gas is doubled, how does the average kinetic energy of its molecules change?

Which of the following gases will have the highest root mean square speed at the same temperature?

Derive the relation between pressure and average kinetic energy per molecule starting from the kinetic theory assumptions.

In a container, two gases A and B are mixed. Gas A has molar mass 4 g/mol and gas B has molar mass 64 g/mol. If both gases are at the same temperature, what is the ratio of their root mean square speeds (v_rms,A / v_rms,B)?

Which of the following statements is NOT true according to kinetic theory of gases?