How does kinetic theory explain gas pressure

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Explanation:

The kinetic molecular theory can be used to explain each of the experimentally determined gas laws. The pressure of a gas results from collisions between the gas particles and the walls of the container. Each time a gas particle hits the wall, it exerts a force on the wall. In the kinetic theory of gases, gas molecules move around in the most random way colliding and bumping into each other and then bouncing off in the opposite direction.

The molecules exert no intermolecular forces on each other and they have no potential energy associated with them in their motion.

Thus the energy is wholly kinetic.

The concept of pressure is explained in kinetic theory as a consequence of kinetic energy of gases. Let me explain it.

Consider an ideal gas (the ones with which kinetic theory is concerned) in a closed container.

Due to the troublesome motion of the gas molecules, they will collide with each other, some of them shall collide with the container walls and then bounce back and this process continues.

Binary chemical compound is a chemical compound that contains exactly two different elements. The two major types of binary chemical compounds are Na+, Mg+2. The three examples of each type of binary compound are  NaCl (sodium chloride), NaF (sodium fluoride), and MgO (magnesium oxide).