The average kinetic energy of gas molecules depends on the absolute temperature of the gas. Let's discuss this in detail:

1. Kinetic Theory of Gases:
The kinetic theory of gases explains the behavior of gases based on the motion of their particles. According to this theory, gas molecules are in constant random motion, and their kinetic energy is directly related to their temperature.

2. Kinetic Energy of Gas Molecules:
The kinetic energy of a gas molecule is the energy associated with its motion. It is given by the equation:

Kinetic energy = (1/2) * mass * velocity^2

Where:
- Mass is the mass of the gas molecule
- Velocity is the speed of the gas molecule

3. Relationship with Temperature:
Temperature is a measure of the average kinetic energy of the gas molecules in a sample. It indicates how fast the gas molecules are moving. The higher the temperature, the faster the gas molecules move, and thus, the greater their average kinetic energy.

4. Relationship with Absolute Temperature:
The absolute temperature of a gas is measured in Kelvin (K) and is proportional to the average kinetic energy of the gas molecules. The relationship between temperature and kinetic energy can be expressed using the following equation:

Average kinetic energy = (3/2) * k * T

Where:
- k is the Boltzmann constant (a constant value)
- T is the absolute temperature in Kelvin

From this equation, it is clear that the average kinetic energy of gas molecules depends directly on the absolute temperature of the gas.

In conclusion, the average kinetic energy of gas molecules depends on the absolute temperature of the gas. As the temperature increases, the average kinetic energy of the gas molecules also increases. Therefore, option 'C' is the correct answer.