Question

We have a gas in a closed container. Say, we put some weight on the lid of the container. This increases the pressure on the container, which in turn causes the gas particles to come close to one another. As a result, the kinetic energy of the particles reduces. Nevertheless, the particles are still quite far away from one another and, hence, are still in gaseous state. When the pressure on the container is increased further, the gas particles come very close to one another. Gradually, the gas liquefies.
if we carefully read this, we find that temperature is somewhat inverse of pressure, because when pressure is increased kinetic energy of particles is decreasing, but if temperature is increased the kinetic energy will also increase.
so, what is causing discrepancy here to the fact that temperature is directly proportional to pressure?

Answer 1

When the pressure is high volume is low and the particles come closer to each other. As it undergoes strong force of attraction, the gas starts liquify. As volume is low temperature is low according to Charles law. So when temperature is low kinetic energy will become lower. At high temperature it starts increasing.