Find the gas,if its density at $273 \ K$ temperature and $76 \ cm \ Hg$ pressure is $1.94 \ g / dm^3$.

Assuming ideal gas behaviour,the ratio of density of ammonia to that of hydrogen chloride at the same temperature and pressure is: (Atomic wt. of $Cl = 35.5 \ u$)

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). $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

$A$ 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 Neon will be highest at

$A$ $10.0 \, L$ flask contains $64 \, g$ of oxygen at $27^{\circ} C$. (Assume $O_2$ gas is behaving ideally). The pressure inside the flask in bar is $.....$
(Given $R = 0.0831 \, L \, bar \, K^{-1} \, mol^{-1}$)