$400 \ cm^{3}$ of oxygen at $27\,^{\circ}C$ were cooled to $-3\,^{\circ}C$ without change in pressure. The contraction in volume will be ............... $cm^{3}$

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? $(R = 0.083\, dm^3\, bar\, K^{-1}\, mol^{-1})$

If $2.5$ moles of an ideal gas at a certain temperature are allowed to expand isothermally and reversibly from an initial volume of $2$ $dm^3$ to $20$ $dm^3$, the work done by the gas is $-16.5$ $kJ$. The temperature (in $K$) of the gas is (Round off to the nearest value). $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

At $0^{\circ} C$,a gas occupies $22.4 \ L$. What is the temperature in Kelvin required to reach a volume of $224 \ L$ (in $K$)?

An open vessel at $27\,^oC$ is heated such that $\frac{3}{5}$ of the air in it is expelled. Assuming the volume of the vessel remains constant,calculate the temperature in $K$ to which the vessel was heated.

At $STP$,$2 \ mol$ of $N_2$ gas in a $50 \ L$ container exhibits: