The lattice energy of sodium chloride crystal is the energy released when 1 mole of NaCl is formed from
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The lattice energy of sodium chloride, $\mathrm{NaCl}$, is $-787.5 \mathrm{kJ} / \mathrm{mol}$ . The lattice energy of potassium chloride, $\mathrm{KCl}$, is $-715 \mathrm{k} / / \mathrm{mol}$ . In which compound is the bonding between ions stronger? Why?
Calculate the free energy change when 1 mole of $\mathrm{NaCl}$ is dissolved in water at $25^{\circ} \mathrm{C}$. Lattice energy of $\mathrm{NaCl}=777.8 \mathrm{~kJ} \mathrm{~mol}^{-1} ; \Delta S$ for dissolution $=0.043 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and hydration energy of $\mathrm{NaCl}=-774.1$ $\mathrm{kJ} \mathrm{mol}^{-1} .$
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