Calculate the work done during compression of $2 \ mol$ of an ideal gas from a volume of $1 \ m^3$ to $10 \ dm^3$ at $300 \ K$ against a constant external pressure of $100 \ kPa.$

$1 \text{ mole}$ of an ideal gas is compressed isothermally and reversibly from an initial pressure $x \text{ kPa}$ to a final pressure $2x \text{ kPa}$ at $300 \text{ K}$. Find the work done $(R = 8.314 \text{ J K}^{-1} \text{mol}^{-1})$. (in $\text{ J}$)

An ideal gas is allowed to expand from $2 \ dm^3$ to $6 \times 10^{-3} \ m^3$ against a constant external pressure of $1 \ bar$. The work done in $kJ$ is (in $kJ$)

If a system neither gains nor loses heat during its transformation from one state to another,such a process is called ......

Out of boiling point $(I)$,entropy $(II)$,$pH$ $(III)$ and $emf$ of a cell $(IV)$,intensive properties are

The change in internal energy $\Delta U$ of an ideal gas depends on: