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.

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

the answer is na (sodium)