Embibe Experts Solutions for Chapter: States of Matter: Gaseous and Liquid states, Exercise 1: Exercise 1

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

Find the density of ${\mathrm{CO}}_2\left(\mathrm{g}\right)$ with respect to ${\mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)$.

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:

The density of acetic acid vapor at $300 \mathrm{K}$ and $1 \mathrm{atm}$ is $5 \mathrm{mg} {\mathrm{cm}}^{-3}$. The number of acetic acid molecules in the cluster that is formed in the gas phase is the closest to 

$10$ moles of a mixture of hydrogen and oxygen gases at a pressure of $1 \mathrm{atm}$ at constant volume and temperature, react to form $3.6 \mathrm{g}$ of liquid water. The pressure of the resulting mixture will be closest to:

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

In the following compressibility factor $\left(\mathrm{Z}\right)$ vs. pressure graph at $300 \mathrm{K}$, the compressibility of ${\mathrm{CH}}_4$ at pressures $<200 \mathrm{bar}$ deviates from ideal behaviour because:

One mole, each of the two gases $\mathrm{X}$ and $\mathrm{Y}$, are stored separately in two cylinders at $25°\mathrm{C}$ at pressures $1 \mathrm{atm}$ and $2 \mathrm{atm}$, respectively. The difference in the compressibilities of the two gases, $\left({\mathrm{k}}_{\mathrm{x}}-{\mathrm{k}}_{\mathrm{y}}\right)$, is: