When $5 \, g$ of $XeF_4$ gas is filled in a $6 \, L$ container at $80 \, ^oC$,the pressure exerted by the gas will be ......... $atm$.

Choose the correct option for the total pressure (in $atm$) in a mixture of $4 \ g$ $O_2$ and $2 \ g$ $H_2$ confined in a total volume of $1 \ L$ at $0^{\circ} C$ is :
$\left[ \text{Given } R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}, T = 273 \ K \right]$

$34.05 \, mL$ of phosphorus vapour weighs $0.0625 \, g$ at $546^{\circ} C$ and $0.1 \, bar$ pressure. What is the molar mass of phosphorus?

What will be the pressure exerted by a mixture of $3.2 \ g$ of methane and $4.4 \ g$ of carbon dioxide contained in a $9 \ dm^3$ flask at $27^{\circ} C$?

$A$ $5.75 \ g$ sample of a gas occupies $3.5 \ L$ at $55 \ ^oC$ and $0.940 \ atm$ pressure. What is the molecular weight of the gas?

The density of a gas at $-23 \ ^oC$ temperature and $780 \ \text{torr}$ pressure is $1.40 \ g/L$. Identify the gas.