Embibe Experts Solutions for Chapter: Gaseous State, Exercise 2: KVPY PROBLEMS (PREVIOUS YEARS)

The ratio of the root-mean-square velocity of hydrogen at $50 \mathrm{K}$ to that of nitrogen at $500 \mathrm{K}$ is the closest to:

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:

According to Graham's Law, the rate of diffusion of $\mathrm{CO}, {\mathrm{O}}_2, {\mathrm{N}}_2$ and ${\mathrm{CO}}_2$ follows the order:

In a closed vessel, an ideal gas at $1 \mathrm{atm}$ is heated from $27°\mathrm{C}$ to $327°\mathrm{C}$. The final pressure of the gas will approximately be:

A reaction has an activation energy of $209 \mathrm{kJ} {\mathrm{mol}}^{-1}$. The rate increases $10$-fold when the temperature is increased from $27°\mathrm{C}$ to $\mathrm{X}°\mathrm{C}$. The temperature $\mathrm{X}$ is closest to:

[Gas constant, $\mathrm{R}=8.314 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}$]

A mixture of toluene and benzene boils at $100°\mathrm{C}$. Assuming ideal behaviour, the mole fraction of toluene in the mixture is closest to:

[Vapour pressures of pure toluene and pure benzene at $100°\mathrm{C}$ are $0.742$ and $1.800 \mathrm{bar}$, respectively. $1 \mathrm{atm}=1.013 \mathrm{bar}$]

The pressure $\left(\mathrm{P}\right)-$volume $\left(\mathrm{V}\right)$ isotherm of a Van der Waals gas, at the temperature at which it undergoes gas to liquid transition, is correctly represented by:

A container of volume $2.24 \mathrm{L}$ can withstand a maximum pressure of $2 \mathrm{atm}$ at $273 \mathrm{K}$ before exploding. The maximum amount of nitrogen (in $\mathrm{g}$) that can be safely put in this container at this temperature is closest to: