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  • Calculate the hydration enthalpy of sodium ion if the lattice energy of sodium chloride is mea

Calculate the hydration enthalpy of sodium ion if the lattice energy of sodium chloride is 200\ \mathrm{k cal/mol } meal. Also, the dissolution of the salt was endothermic upto 1.5\ \mathrm{k cal/mol} and 5:4 was the ratio of hydration energies of sodium and the chloride ion.

Option: 1

100.27\ \mathrm{kcal} / \mathrm{mol}


Option: 2

-110.27\ \mathrm{kcal} / \mathrm{mol}


Option: 3

58.97\ \mathrm{kcal} / \mathrm{mol}


Option: 4

-58.97\ \mathrm{kcal} / \mathrm{mol}


Answers (1)

best_answer

\begin{aligned} \Delta H_{\text {sol }} & =\Delta H_{\text {hyd }}+\Delta H_{\text {latice }} \\ 1.5 & =\Delta H_{\text {hyd }}+200 \\ \Delta H_{\text {hyd }} & =-198.5\ \mathrm{kcal} / \mathrm{mal} \end{aligned}
\begin{aligned} \Delta H_{\text {hyd }}\left(\mathrm{Na}^{+}\right) & \neq \Delta H_{\text {hyd }}\left(\mathrm{C}^{-}\right)=-198.5 \\ \Delta H_{\text {hyd }}\left(\mathrm{Na}^{+}\right) & =-198.5 \times \frac{5}{9} \\ & =-110.27\ \mathrm{kcal} / \mathrm{mol} \end{aligned}

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