As per the kinetic theory of gases, the average kinetic energy of gas molecules is directly proportional to the temperature of the gas. This shows that kinetic energy and temperature are related to each other. The energy of motion that particles possess is called kinetic energy, and the average kinetic energy of the particles within the substance is called temperature.
Molecules in gases are moving and breaking each other, as well as the container walls. With the increase in temperature, the gas molecules’ average K.E. increases. This shows that the molecules are moving faster on average, which results in larger and more intense collisions.
Subsequently, the energy transferred in the collisions generates heat and causes the temperature of the gas to increase. At the other end, however, when temperatures go down, there is a decrease in the average K.E. of the molecules. This enables them to move slowly as well as strike infrequently, which ends up reducing the temperature.
In short, kinetic energy is directly linked to temperature, especially in gases. The rise in temperature is in accordance with the increase in average K.E. of gas molecules, and the phenomenon also works the other way around.