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Carefullyobserve the given diagrams which indicates standard enthalpyof formation of different states of one mole \( \mathrm{Mg} \) and 2 mole \( \mathrm{Cl} \) atom and match the entries in column I and II provided.
\( P \)
\( \begin{array}{rlc}\text { Energy }(\mathrm{kJ}) \uparrow & \text { State of } \mathrm{Mg}^{2} \text { and } \mathrm{Cl}_{2} \\ +2600 & & {\left[\mathrm{Mg}^{2+}(\mathrm{g})+2 \mathrm{Cl}_{(\mathrm{g})]}\right.} \\ +2360 & {\left[\mathrm{Mg}^{2+}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g})\right]} \\ +1870 & {\left[\mathrm{Mg}^{2+}(\mathrm{g})+2 \mathrm{Cl}^{-}(\mathrm{g})\right]} \\ & & {\left[\mathrm{Mg}^{2+}(\mathrm{g})+2 \mathrm{Cl}^{-}(\mathrm{aq})\right]} \\ +1110 & & {\left[\mathrm{Mg}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g})\right]} \\ & +170 & {\left[\mathrm{Mg}^{(\mathrm{s})}+\mathrm{Cl}_{2}(\mathrm{~g})\right]} \\ 0 & -640 & {\left[\mathrm{MgCl}_{2}(\mathrm{~s})\right]} \\ -790 & {\left[\mathrm{Mg}^{2+}(\mathrm{aq})+2 \mathrm{Cl}_{(\mathrm{aq})}\right)} \\ \text { Column II }\end{array} \)
Column I
(P) \( -1900 \mathrm{~kJ} / \mathrm{mol} \)
(A) \( \Delta \mathrm{H}_{\mathrm{f}}\left[\mathrm{Mg}^{2+}(\mathrm{aq})\right] \)
(Q) \( \quad+460 \mathrm{~kJ} / \mathrm{mol} \)
(B) \( \Delta \mathrm{H}_{\mathrm{f}}\left[\mathrm{Cl}^{-}(\mathrm{aq})\right] \)
(R) \( -625 \mathrm{~kJ} / \mathrm{mol} \)
(C) \( \Delta \mathrm{H}_{\text {hydration }}\left[\mathrm{Mg}^{2+}(\mathrm{g})\right] \)
(S) \( \quad+2510 \mathrm{~kJ} / \mathrm{mole} \)
(D)(D) \( \quad \mid \) L.E. \( \mathrm{MgCl}_{2}(\mathrm{~s}) \mid \)
L.E. = Lattice enthalpy
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