The temperature at which $4 \ mol$ of a gas occupies $5 \ dm^3$ volume at $3.32 \ bar$ pressure is:

The value of the universal gas constant $R$ is:

At $25 \, ^\circ C$ temperature and $760 \, mm \, Hg$ pressure,the volume of a gas is $600 \, mL$. Calculate the pressure when the volume of this gas becomes $640 \, mL$ at $10 \, ^\circ C$ temperature. Use the ideal gas equation: $\frac{p_1 V_1}{T_1} = \frac{p_2 V_2}{T_2}$

One mole of an ideal gas occupies $12 \ L$ at $297^{\circ} C$. What is the pressure of the gas?

Calculate the pressure of $HCl$ gas having a density of $8 \, kg \, m^{-3}$ at a temperature of $-40 \, ^oC$. (Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$,Molar mass of $HCl = 36.5 \, g \, mol^{-1} = 0.0365 \, kg \, mol^{-1}$)

Which gas has a density of $1.24 \ g/L$ at $0^{\circ} C$ and $1 \ atm$ pressure?