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, $$R=8.314 \mathrm{~JK}^{-1} \mathrm{~mol}^{-1}$$ )

1 mole of $$\mathrm{CO}_2$$ gas at $$300 \mathrm{~K}$$ is expanded under adiabatic conditions such that its volume becomes 27 times. What is work done?

In thermodynamics, a quantity whose value simply depends upon the initial and final state of the system is called