If two moles of an ideal gas at $546 \ K$ occupy a volume of $44.8 \ L$,the pressure must be ............. $atm$.

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 gas equation $PV = nRT$ is applicable for which of the following conditions?

The $S.I.$ unit of the gas constant $R$ is:

One mole of an ideal gas occupies $12 \ L$ at $297^{\circ} C$. What is the pressure of the gas?

At $0\, ^\circ C$ and $1\, \text{atm}$ pressure,a gas occupies $100\, \text{cc}$. If the pressure is increased to $1.5$ times and the temperature is increased by one-third of its absolute temperature,then the final volume of the gas will be :- $cc$