S C Kheterpal, S N Dhawan and, P N Kapil Solutions for Chapter: States of Matter: Gases and Liquids, Exercise 4: PROBLEMS FOR PRACTICE

Calculate the number of moles of hydrogen gas present in $500 {\mathrm{cm}}^3$ of the gas taken at $300 \mathrm{K}$ and $760 \mathrm{mm}$ pressure. If this sample of hydrogen is found to have a mass equal to $4.09\times {10}^{-2} \mathrm{g}$, calculate the molar mass of hydrogen.

$2.802 \mathrm{g}$ of ${\mathrm{N}}_2$ gas is kept in a litre flask at $0°\mathrm{C}$. Calculate the pressure exerted by the gas.

Calculate the molar volume of a gas at STP.

A $500 \mathrm{mL}$ sample of a gas weighs $0.326 \mathrm{g}$ at $100°\mathrm{C}$ and $0.500 \mathrm{atm}$. What is the molecular mass of the gas?

A large flask fitted with a stop-cock is evacuated and weighed; its mass is found to be $134.567 \mathrm{g}$. It is then filled to a pressure of $735 \mathrm{mm}$ at $31°\mathrm{C}$ with a gas of unknown molecular mass and then reweighed; its mass is $137.456 \mathrm{g}$. The flask is then filled with water and weighed again; its mass is now $1067.9 \mathrm{g}$. Assuming that the gas is ideal, calculate the molar mass of the gas.