What will be the volume in $L$ of $2.8 \ g$ of carbon monoxide at $27 \ ^oC$ temperature and $0.821 \ atm$ pressure? $(R = 0.0821 \ L \ atm \ mol^{-1} K^{-1})$

The density of methane at $27\,^oC$ and $2.0\,atm$ pressure is ............ $g\,L^{-1}$.

At $27\,^oC$ temperature,$4\,mol$ $Cl_2$,$4\,mol$ $N_2$,and $2\,mol$ $O_2$ are filled in a $5\,L$ closed vessel. Find the total pressure of the gaseous mixture. $(R = 8.34 \times 10^{-2} \,bar \,L \,mol^{-1} \,K^{-1})$ (in $,bar$)

In a closed vessel,an ideal gas at $1 \, atm$ is heated from $27^{\circ} C$ to $327^{\circ} C$. The final pressure of the gas will approximately be $..... \, atm$

What is the volume in $litre$ occupied by $7 \, g$ of $N_2$ gas at $27 \, ^oC$ temperature and $750 \, mm \, Hg$ pressure?

The density of gas $A$ is twice that of gas $B$ at the same temperature. The molecular weight of gas $B$ is twice that of gas $A$. The ratio of the pressure of gas $A$ to gas $B$ will be: