How does kinetic theory explain gas pressure

Hope this helps :)

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.

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer