In addition, temperature affects the pressure of gases - a higher pressure occurs in a cylinder with a heated sun than in the same cylinder when immersed in cold water. Understanding the behavior of gases and the concept of pressure is possible thanks to the kinetic theory of gases. You probably remember that kinetic energy is mechanical energy movement. Gases behave in a certain way due to the movement of their molecules.

The kinetic energy of a gas molecule depends on its speed associated with temperature and mass, depending on the type of substance. Larger, faster moving particles of heavier gases exert more force on impact. As you learned earlier, temperature is a measure of how fast particles move; The higher the temperature, the faster the particles move, the more likely they are to hit objects - and exert more pressure.

What may seem interesting is that gases with molecules of different masses, but with the same heat, exert the same pressure on the walls. Higher molecular weight molecules move more slowly, so they add up the same wall pressure as lower molecular weight gases moving with more high speed. Temperatures are different. For example, in a light gas such as helium, after a certain amount of heat is applied, the particles are accelerated to a greater extent than in heavier oxygen. However, the pressure change will be the same.

The heavier oxygen, whose molecules move much more slowly, exerts the same pressure due to the increase in molecular weight. Different gases at the same temperature and pressure maintain this relationship between the speed and mass of the molecule. Particles in lighter gases move faster. It follows from the kinetic theory of gases that the gas fraction at certain temperature has kinetic energy like the same number of other gas molecules at the same temperature.