Chapter 10, Problem 97AP

Interpretation Introduction

Interpretation: To find which among the given gases behaves most ideally under the same conditions of temperature and pressure.

Concept introduction:

The kinetic molecular theory is based on four assumptions that describe the behavior of gases. They are as follow:

The molecules of a gas are loosely packed and so the volume occupied by the molecules of a gas is negligible.

The molecules of gases move in a random manner and collide with external materials and with one another without loss of energy, that is, elastic collision.

Their molecules do not attract or repel each other.

The average kinetic energy of gas molecules is in direct proportionality to the absolute temperature of the molecules. Therefore,

$\overline{{\text{E}}_{\text{k}}}\infty \text{ T}$

The general ideal gas equation is as follows:

$PV=nRT$

Van der Waal’s equation for real gases is as follows:

$\left(P+\frac{a{n}^2}{V^2}\right)\left(V-nb\right)=nRT$

Here, $P$ is the pressure of ideal gas, $V$ is the volume of ideal gas, $n$ is the number of molecules, $a,b$ are proportionality constants, $R$ is gas constant, and $T$ is the absolute temperature.

And, $\frac{a{n}^2}{V^2}$ and $nb$ are the corrective terms for pressure and volume, respectively.