$A$ certain system is exothermic by $260 \ kJ$ and does $10 \ kJ$ of work. What is the change in internal energy (in $kJ$)?

$\Delta_{vap} H^{\ominus}$ for water is $+40.49 \ kJ \ mol^{-1}$ at $1 \ bar$ and $100^{\circ} C$. The change in internal energy for this vaporization under the same conditions is . . . . . . . . . . $kJ \ mol^{-1}$. (Integer answer) (Given $R = 8.3 \ J \ K^{-1} \ mol^{-1}$)

For water $\Delta_{vap} H = 41 \ kJ \ mol^{-1}$ at $373 \ K$ and $1 \ bar$ pressure. Assuming that water vapour is an ideal gas that occupies a much larger volume than liquid water,the internal energy change during evaporation of water is $...... \ kJ \ mol^{-1}$.
[Use: $R = 8.3 \ J \ mol^{-1} \ K^{-1}$]

$A$ gas absorbs $120 \text{ J}$ of heat and expands by $300 \times 10^{-6} \text{ m}^3$ against a constant external pressure of $2 \times 10^5 \text{ Nm}^{-2}$. What will be the change in internal energy of the system (in $\text{ J}$)?

$A$ piston filled with $0.04 \ mol$ of an ideal gas expands reversibly from $50.0 \ mL$ to $375 \ mL$ at a constant temperature of $37.0 \ ^oC$. As it does so,it absorbs $208 \ J$ of heat. The values of $q$ and $w$ for the process will be
$(R = 8.314 \ J/mol \ K) \ (\ln 7.5 = 2.01)$

For water at $100^{\circ} C$ and $1 \, bar$,$\Delta_{vap} H - \Delta_{vap} U = ...... \times 10^{2} \, J \, mol^{-1}$. (Round off to the Nearest Integer) $[Use : R = 8.31 \, J \, mol^{-1} \, K^{-1}]$ [Assume volume of $H_{2}O_{(\ell)}$ is much smaller than volume of $H_{2}O_{(g)}$. Assume $H_{2}O_{(g)}$ treated as an ideal gas]