Question

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Answer 1

1.The kinetic-molecular theory of gases can be stated as four postulates: A gas consists of molecules in constant random motion. Gas molecules influence each other only by collision; they exert no other forces on each other. All collisions between gas molecules are perfectly elastic; all kinetic energy is conserved.

2.the value of volume we calculated is less than the actual practical volume. Hence from the above two graphs, it is clear that generali real gases, under all conditions do not follow The Ideal Gas Behaviour or equation.

3.Real gases are nonideal gases whose molecules occupy space and have interactions; consequently, they do not adhere to the ideal gas law.

4.At low temperatures or high pressures, real gases deviate significantly from ideal gas behavior. ... The kinetic theory assumes that gas particles occupy a negligible fraction of the total volume of the gas. It also assumes that the force of attraction between gas molecules is zero.

5.Vander Waal pointed out that following two assumptions in kinetic theory are faulty: (i) The volume occupied by the gas molecule is negligible in comparison to the total volume of the gas. This assumption is nearly valid if the pressure is low. (ii) The molecules do not exert any force of attraction upon one another.

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Answer 2

Explanation:

Real gases are nonideal gases whose molecules occupy space and have interactions; consequently, they do not adhere to the ideal gas law.