At $300 \ K$ temperature,the pressure of $2.5 \ g$ of $N_2$ gas is $4 \ bar$ and its volume is $2.5 \ L$. If the pressure becomes $10 \ bar$ at the same temperature,calculate its new volume. (in $L$)

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 :
$\left[ \text{Given } R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}, T = 273 \ K \right]$

At what temperature in $^\circ C$ will the volume of a gas become double its volume at $0\,^\circ C$?

For an ideal gas,the compressibility factor $(Z)$ is equal to:

Pressure of a mixture of $4 \ g$ of $O_2$ and $2 \ g$ of $H_2$ confined in a bulb of $1 \ L$ at $0^{\circ}C$ is $..... \ atm$

What is the compressibility factor of an ideal gas?