$A$ certain mass of a gas occupies a volume of $2 \,L$ at $STP$. To what temperature must the gas be heated to double its volume, keeping the pressure constant?

Equal amounts of gases are kept in two separate containers. If the densities of the two gases are in $1:2$ ratio and their temperatures are in $2:1$ ratio, calculate the ratio of their respective pressures.

At a given temperature,the density of an ideal gas is proportional to $(P = \text{pressure of ideal gas})$

At $300\, K$,the density of a certain gaseous molecule at $2\, bar$ is double that of dinitrogen $(N_2)$ at $4\, bar$. The molar mass of the gaseous molecule is ............... $g\, mol^{-1}$.

$A$ monoatomic ideal gas,initially at temperature $T_1$,is enclosed in a cylinder fitted with a frictionless piston. The gas is allowed to expand adiabatically to a temperature $T_2$ by releasing the piston suddenly. $L_1$ and $L_2$ are the lengths of the gas columns before and after the expansion,respectively. The ratio $\frac{T_2}{T_1}$ is:

At $25 \, ^\circ C$,a $3.7 \, g$ gas occupies the same volume as $0.184 \, g$ of $H_2$ gas at $17 \, ^\circ C$ under the same pressure. What is the molar mass of the gas?