An ideal gas is allowed to expand from $1 \, L$ to $10 \, L$ against a constant external pressure of $1 \, bar$. The work done in $kJ$ is

$1 \, mol$ of an ideal gas is compressed reversibly at a constant temperature of $27 \, ^oC$ from $1 \, bar$ to $4 \, bar$. Calculate the work done in $kJ$.

What is the value of the standard enthalpy of formation of dihydrogen $(H_2)$?

Expansion of a gas in vacuum is called free expansion. Calculate the work done and the change in internal energy when $1 \ L$ of ideal gas expands isothermally into vacuum until its total volume is $5 \ L$?

In an irreversible expansion of a gas,the work done by the gas is given by.....

What is the enthalpy change (in $J$) for converting $9 \ g$ of $H_2O(l)$ at $+10^{\circ}C$ to $H_2O(l)$ at $+20^{\circ}C$? $(C_p(H_2O(l)) = 75 \ J \ mol^{-1} \ K^{-1})$