Explanation:

Absolute temperature:
- The average kinetic energy of a gas molecule is directly proportional to the absolute temperature of the gas.
- As the temperature of the gas increases, the average kinetic energy of the gas molecules also increases.
- This is because temperature is a measure of the average kinetic energy of the particles in a substance.

Volume of gas:
- The volume of gas does not directly affect the average kinetic energy of a gas molecule.
- However, changes in volume can affect the pressure of the gas, which in turn can affect the temperature of the gas, thereby indirectly influencing the average kinetic energy of the gas molecules.

Molar mass:
- The molar mass of the gas molecules does not directly affect the average kinetic energy of a gas molecule.
- However, lighter gas molecules tend to have higher average kinetic energies compared to heavier gas molecules at the same temperature.
- This is because lighter gas molecules have higher velocities due to their lower mass.

Mass of the gas taken:
- The mass of the gas taken does not directly affect the average kinetic energy of a gas molecule.
- The number of gas molecules present in the sample and the temperature of the gas are the main factors that determine the average kinetic energy of the gas molecules.

In conclusion, the average kinetic energy of a gas molecule depends mainly on the absolute temperature of the gas. Changes in temperature will directly affect the average kinetic energy of the gas molecules, while other factors such as volume, molar mass, and mass of the gas taken can indirectly influence the average kinetic energy through their effects on temperature and pressure.