When the temperature of a flask with a capacity of $1 \ L$ is increased from $25 \ ^oC$ to $35 \ ^oC$,calculate the volume of air in $mL$ that escapes from the flask.

The volume of a given amount of gas at $27^{\circ} C$ at constant pressure is $420 \ cm^3$. If the temperature is reduced by $20^{\circ} C$ at constant pressure, what will be the volume of the gas (in $cm^3$)?

The volume occupied by $1.8 \; g$ of water vapour at $374^{\circ} C$ and $1 \; bar$ pressure will be $....... \; L$ : [Use $R=0.083 \; bar \; L \; K^{-1} \; mol^{-1}$]

Volume of a given mass of gas at $17 \, ^oC$ is measured as $200 \, cm^3$. The volume of the same mass of that gas at same pressure and at temperature of $47 \, ^oC$ will be .............. $cm^{3}$

What is the numerical value of gas constant $R$ in terms of $L \ atm \ K^{-1} \ mol^{-1}$?

When $2 \ g$ of a gaseous substance $A$ is introduced into an initially evacuated flask at $25^{\circ} C$,the pressure is found to be $1 \ atm$. $3 \ g$ of another gaseous substance $B$ is added to it at the same temperature and pressure. The final pressure is found to be $1.5 \ atm$. Assuming ideal gas behaviour,the ratio of molar masses of $A$ and $B$ is: