$A$ sample of oxygen gas and a sample of hydrogen gas both have the same mass,same volume,and the same pressure. The ratio of their absolute temperatures is (Molecular weights of $O_2$ and $H_2$ are $32$ and $2$ respectively).

The gas in a vessel is subjected to a pressure of $20 \ atm$ at a temperature of $27^{\circ}C$. If one-half of the gas is released from the vessel and the temperature of the remaining gas is raised by $50^{\circ}C$,the final pressure of the gas in the vessel is ....... $atm$.

What is the value of the volume of an ideal gas at absolute zero temperature?

The equation of state for $n$ moles of an ideal gas is $PV = nRT$, where $R$ is a constant. The $SI$ unit for $R$ is

Gas at pressure $P$, temperature $T$, and volume $V$ is filled in jar $A$. Another jar $B$ is filled with gas having parameters $2P, \frac{V}{4}, 2T$. The ratio of the number of molecules of jar $B$ to those of jar $A$ is:

The pressure and temperature of an ideal gas in a closed vessel are $720 \, kPa$ and $40^\circ C$ respectively. If $\frac{1}{4}^{th}$ of the gas is released from the vessel and the temperature of the remaining gas is raised to $353^\circ C$,the final pressure of the gas is ....... $kPa$.