$A$ gas occupies $100 \, cc$ volume at $0 \, ^oC$ temperature and $1 \, atm$ pressure. If the pressure is increased by $1.5$ times and the temperature is increased by one-third of its absolute temperature,what will be the final volume of the gas in $cc$?

At what temperature in $K$ will $28 \ g$ of $N_2$ gas occupy a volume of $10.0 \ L$ at $2.46 \ atm$ pressure?

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.

For $1 \ mol$ of an ideal gas,an isochore is obtained. The slope of the isochore is $0.082 \ atm \ K^{-1}$. What will be its pressure (in $atm$) when the temperature is $12.2 \ K$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$.

$A$ sealed flask with a capacity of $2 \, dm^{3}$ contains $11 \, g$ of propane gas. The flask is so weak that it will burst if the pressure becomes $2 \, MPa$. The minimum temperature at which the flask will burst is $....... \, ^{\circ}C$. [Nearest integer] (Given: $R = 8.3 \, J \, K^{-1} \, mol^{-1}$. Atomic masses of $C$ and $H$ are $12 \, u$ and $1 \, u$ respectively.) (Assume that propane behaves as an ideal gas.)

$A$ vacuum vessel of volume $1 \, dm^3$ is evacuated at a constant temperature of $-23 \, ^\circ C$ until the pressure drops to $7.6 \times 10^{-5} \, torr$. What is the number of molecules remaining in the vessel?