JEE Mains · Chemistry · STD 11 - 5. Thermodynamics and thermochemistry
The hydration energies of \(\mathrm{K}^{+}\)and \(\mathrm{Cl}^{-}\)are -x and -y \(\mathrm{kJ} / \mathrm{mol}\) respectively. If lattice energy of KCl is -z \(\mathrm{kJ} / \mathrm{mol}\), then the heat of solution of KCl is what?
- A \(+x-y-z\)
- B \(x+y+z\)
- C \(z-(x+y)\)
- D \(-\mathrm{z}-(\mathrm{x}+\mathrm{y})\)
Answer & Solution
Correct Answer
(C) \(z-(x+y)\)
Step-by-step Solution
Detailed explanation
\begin{aligned} \Delta \mathrm{H}_{\text {Sol}^{\mathrm{n}}.} & =\mathrm{L} \cdot \mathrm{E} \cdot+(\mathrm{H} \cdot \mathrm{E})_{\mathrm{K}_{(\mathrm{g})}^{+}}+(\mathrm{HE})_{\mathrm{Cl}_{(\mathrm{g})}^{-1}} \\ & =\mathrm{Z}-\mathrm{x}-\mathrm{y} \\ &…
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