$A$ $2.24\,L$ oxygen cylinder shows a leakage at $NTP$. When the leakage is plugged,the pressure drops by $570\,mm\,Hg$. What is the number of moles of gas that escaped?

Calculate the temperature of $4.0 \, mol$ of a gas occupying $5 \, dm^{3}$ at $3.32 \, bar$.
$(R = 0.083 \, bar \, dm^{3} \, K^{-1} \, mol^{-1})$

$A$ gas is present at a pressure of $2 \,atm$. What should be the increase in pressure, so that the volume of the gas can be decreased to $\frac{1}{4}$ of the initial volume at constant temperature (in $\,atm$)?

At a temperature of $300 \ K$,if the pressure of $0.09 \ mol$ of a gas is halved,what will be its volume?

What is the effect of temperature change on the Boyle's law isotherm graph?

At $300 \ K$,a sample of $3.0 \ g$ of gas $A$ occupies the same volume as $0.2 \ g$ of hydrogen $(H_2)$ at $200 \ K$ at the same pressure. The molar mass of gas $A$ is $...... \ g \ mol^{-1}$ (nearest integer). Assume that the gases behave as ideal gases.