$A$ certain sample of gas has a volume of $0.2 \ L$ measured at $1 \ atm$ pressure and $0 \ ^oC$. At the same pressure but at $273 \ ^oC$,its volume will be ................ $L$.

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

Explain the relationship between the moles of a gas,its volume,and its density.

$A$ box contains $0.90 \ g$ of liquid water in equilibrium with water vapour at $27^{\circ} C$. The equilibrium vapour pressure of water at $27^{\circ} C$ is $32.0 \ Torr$. When the volume of the box is increased,some of the liquid water evaporates to maintain the equilibrium pressure. If all the liquid water evaporates,then the volume of the box must be $.... \ litre$. [nearest integer]
(Given $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$)
(Ignore the volume of the liquid water and assume water vapours behave as an ideal gas.)

State Avogadro's Law and Gay-Lussac's Law.

Find the moles of $O_2$ having pressure $250 \ bar$ in $500 \ mL$ vessel at $300 \ K$ temperature. $[R = 8.314 \times 10^{-2} \ bar \ L \ K^{-1} \ mol^{-1}]$