Embibe Experts Solutions for Chapter: States of Matter, Exercise 1: Exercise 1

The plot that is not valid for an ideal gas where $\mathrm{P}$ is the pressure and $\mathrm{V}$ is the volume of the gas is:

For an ideal gas, Boyle's law is best described by -

Two balloons, $\mathrm{A}$ and $\mathrm{B}$, containing $0.2$ mole and $0.1$ mole of helium at room temperature and $2.0 \mathrm{atm}$., respectively, are connected. When an equilibrium is established, the final pressure of $\mathrm{He}$ in the system is:

At $298 \mathrm{K}$, assuming ideal behaviour, the average kinetic energy of a deuterium molecule is:

Compressibility factor for ${\mathrm{H}}_2$ behaving as real gas is:

At low pressures (For $1$ mole), the Van der Waal's equation is written as

$\left[\mathrm{p}+\frac{\mathrm{a}}{{\mathrm{V}}^2}\right]\mathrm{V}=\mathrm{RT}$.

The compressibility factor is then equal to:

The values of Van der Waals constant, ${}^{\text{'}\text{'}}\mathrm{a}^{\text{'}\text{'}}$, for the gases ${\mathrm{O}}_2, {\mathrm{N}}_2, {\mathrm{NH}}_3 \& {\mathrm{CH}}_4$ are $1.36, 1.39, 4.17, 2.253 {\mathrm{L}}^2 \mathrm{atm} {\mathrm{mole}}^{-2}$, respectively. The gas which can most easily be liquefied is:

An ideal gas is subjected to a cyclic change as shown in the $\mathrm{P}-\mathrm{V}$ diagram below:

The step in which the gas will cool down is along: