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

Oxygen and cyclopropane at partial pressures of $570 \mathrm{torr}$ and $170 \mathrm{torr}$, respectively, are mixed in a gas cylinder. What is the ratio of the number of moles of cyclopropane to the number of moles of oxygen?

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:

The gas that has the slowest rate of diffusion among ${\mathrm{O}}_2, {\mathrm{H}}_2, {\mathrm{CO}}_2$ and ${\mathrm{CH}}_4$ is:

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:

If a gas is allowed to expand at constant temperature then which of the following is true:

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:

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

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