Identify the incorrect statements among the following:

(a) All enthalpies of fusion are positive

(b) The magnitude of enthalpy change does not depend on the strength of the intermolecular interactions in the substance undergoing phase transformations.

(c) When a chemical reaction is reversed, the value of $\Delta \mathrm{rH}^{\circ}$ is reversed in sign.

(d) The change in enthalpy is dependent of path between initial state (reactants) and final state (products)

(e) For most of the ionic compounds, $\Delta_{\text {sol }} \mathrm{H}^{\circ}$ is negative

From the diagram $(Z)=\frac{V_{\text {real }}}{V_{\text {ideal }}}$

$\Delta_r H$ for the reaction, $C \rightarrow A$ is

A gas at a pressure of $$2 \mathrm{~atm}$$ is heated from $$25^{\circ} \mathrm{C}$$ to $$323^{\circ} \mathrm{C}$$ and simultaneously compressed of $$\frac{2}{3}$$rd of its original value. Then the final pressure is

Lattice enthalpy for $$\mathrm{NaCl}$$ is $$+788 \mathrm{~kJ} \mathrm{~mol}^{-1}$$ and $$\Delta H_{\text {hyd }}^{\circ}=-784 \mathrm{~kJ} \mathrm{~mol}^{-1}$$. Enthalpy of solution of $$\mathrm{NaCl}$$ is