Calculate the volume in liters for $7 \ g$ of $O_2$ gas at $27 \ ^\circ C$ and $750 \ mm$ of $Hg$ pressure.

If the absolute temperature of an ideal gas becomes double and the pressure becomes half,the volume of the gas would be:

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

$A$ gas occupies a volume of $0.35 \ dm^3$ at $290 \ K$ and $2 \ atm$ pressure. Calculate the volume of the gas at $STP$. (in $dm^3$)

An ideal gas on isothermal reversible compression from $10 \ L$ to $5 \ L$ performs $1730 \ J$ of work at $300 \ K$. Calculate the number of moles of gas involved in the compression? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

The density of ammonia gas at $27^{\circ}C$ and $3 \, atm$ pressure is approximately: