Ramendra C Mukerjee Solutions for Chapter: Properties of Gases, Exercise 2: Objective Problems

If the product of the gas constant $\mathrm{R}$i.e., $.0821$$\mathrm{L} \mathrm{atm}/\mathrm{K}/\mathrm{mole}$ and $\mathrm{NTP}$ temperature in kelvin equals $22.4,$ the compressibility factor of the gas at $1$ atmospheric pressure is

The graph of the quantity $\mathrm{d}/\mathrm{p}$ against pressure is extrapolated to zero pressure to obtain a limiting value. If, this limiting $\mathrm{d}/\mathrm{p}$ value for a certain non-ideal gas is found to be $2.86 \mathrm{g}/\mathrm{L}-\mathrm{atm}$ at $0°\mathrm{C}$, the molar mass of the gas will be:

The root mean square speed of ${\mathrm{N}}_2$ molecules in a gas sample can be changed by:

How high must a column of water be to exert a pressure equal to that of a column of $\mathrm{Hg}$, that is $760 \mathrm{mm}$ high

In the following graph in which volume is plotted versus temperature, the lines $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$, represent the same mass of the same ideal gas at different pressures ${\mathrm{p}}_1, {\mathrm{p}}_2$ and ${\mathrm{p}}_3$, respectively.

The correct relationship of pressures is

A $5.0 \mathrm{L}$ reaction vessel contain hydrogen at a partial pressure of $0.588 \mathrm{atm}$ and oxygen gas at a partial pressure of $0.302 \mathrm{atm}$. The limiting reactant in the following reaction: $2{\mathrm{H}}_2+{\mathrm{O}}_2=2{\mathrm{H}}_2\mathrm{O}$ is:

When a gas is passed through a small hole at a temperature greater than its critical temperature, Joule-Thomson effect will show:

Which of the following statements is wrong?