Use the deviation from the Ideal Gas Equation to explain how increasing the numb

Question

Use the deviation from the Ideal Gas Equation to explain how increasing the number of molecules in an area effects (a) the pressure of a gas and (b) the volume of a gas, then (c) list some of the initial assumptions of the Kinetic Molecular Theory of Gases and (d) explain the deviation in the physical properties observed in gases under extreme cold temperatures and under high density by using van der Waals molecular attractions descriptions of what happens to the kinetic energy and structure atoms and molecules to be able to physically change properties. (P + an^2/V^2) (V - nb) - nRT

Explanation / Answer

a) increasing the number of gas particles results in increased pressure (of the same volume at the same temperature).

c) 1. The volume occupied by the individual particles of a gas is negligible compared to the volume of the gas itself.

2. The collisions exhibited by gas particles are completely elastic; when two molecules collide, total kinetic energy is conserved.

3. The particles of an ideal gas exert no attractive forces on each other or on their surroundings.
4. These molecules are in constant, random, and rapid motion.

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