Under isothermal condition, a gas at 300 K expands from 0.1 L to 0.25 L against a constant external pressure of 2 bar. The work done by the gas is (Given that, 1 L bar $=100 \mathrm{~J}$ )

Given, $\Delta G^{\circ}=-502 \mathrm{~kJ} \mathrm{~mol}^{-1}$ for the dissociation of ,

$\mathrm{Mg}(\mathrm{OH})_2(s) \rightleftharpoons \mathrm{Mg}^{2+}(a q)+2 \mathrm{OH}^{-}(a q)$ at 298 K . Find the $K_{\mathrm{sp}}$ value.

$(R=8314 \mathrm{~J} / \mathrm{mol} \cdot \mathrm{K})$

The bond dissociation energies for $\mathrm{Cl}_2, \mathrm{I}_2$ and ICl are $242.3,151.0$ and $211.3 \mathrm{~kJ} / \mathrm{mol}$ respectively. The enthalpy of sublimation of iodine is $62.8 \mathrm{~kJ} / \mathrm{mol}$. What is the standard enthalpy of formation of $\operatorname{ICl}(\mathrm{g})$ nearly equal to?

The value of $$\Delta E$$ for combustion of $$32 \mathrm{~g}$$ of $$\mathrm{CH}_4$$ is $$-1770778 \mathrm{~J}$$ at $$298 \mathrm{~K}$$. The $$\Delta H$$ combustion for $$\mathrm{CH}_4$$ in $$\mathrm{J} \mathrm{~mol}^{-1}$$ at this temperature will be (Given that, $$R=8.314 \mathrm{~JK}^{-1} \mathrm{~mol}^{-1}$$ )