The temperature of $1 \, mol$ of a gas is increased by $2 \, ^oC$ at constant pressure. The work done will be:

Volume of $0.5 \ mole$ of a gas at $1 \ atm$ pressure and $273 \ K$ is ............. $litres$.

Pressure of a mixture of $4 \ g$ of $O_2$ and $2 \ g$ of $H_2$ confined in a bulb of $1 \ L$ at $0^{\circ}C$ is $..... \ atm$

At $T$ $K$,an ideal gas $(Z)$ present in $V$ $L$ flask exerted a pressure of $16.4$ $atm$. Its concentration is $1$ $mol$ $L^{-1}$. What is the value of $T$ in $K$?

The value of the compressibility factor for an ideal gas is ........ .

At $400 \ K$, an ideal gas is enclosed in a $0.5 \ m^3$ vessel at a pressure of $203 \ kPa$. What is the change in temperature required (in $K$), if it occupies a volume of $0.2 \ m^3$ under a pressure of $304 \ kPa$? (Nearest integer)