At very low pressure,the compressibility factor $Z$ of a $CO_2$ gas with constant molar volume is:

The compressibility factor $(Z)$ for an ideal gas is ...... .

$4.4 \ g$ of a gas at $0^{\circ} C$ and $0.82 \ atm$ pressure occupies a volume of $2.73 \ L$. The gas can be:

$A$ 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:

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

At $21\, ^oC$ temperature,the volume of $212\, g$ of $O_2$ gas is $34\, dm^3$. If the pressure of the gas becomes $1.24\, bar$,then how many grams of $O_2$ gas are left in the container? $(R = 0.083\, dm^3\, bar\, K^{-1}\, mol^{-1})$