The hydration energies of K^{+} and Cl^{-} ar | vedclass

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Question

(C) According to the Born-Haber cycle for the dissolution of an ionic solid,the heat of solution $(\Delta H_{sol})$ is the sum of the lattice energy $

Vedclass · Accepted Answer

$z-(x+y)$

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(C) According to the Born-Haber cycle for the dissolution of an ionic solid,the heat of solution $(\Delta H_{sol})$ is the sum of the lattice energy $(L.E.)$ and the hydration energies $(H.E.)$ of the constituent ions.$\Delta H_{sol} = L.E. + (H.E.)_{K^{+}} + (H.E.)_{Cl^{-}}$Given:$L.E. = -z \ kJ / mol$$(H.E.)_{K^{+}} = -x \ kJ / mol$$(H.E.)_{Cl^{-}} = -y \ kJ / mol$Substituting these values into the equation:$\Delta H_{sol} = (-z) + (-x) + (-y)$$\Delta H_{sol} = -z - x - y$$\Delta H_{sol} = -(z + x + y)$Wait,let us re-evaluate the standard definition. Usually,$L.E.$ is defined as the energy released when gaseous ions form a solid,so $L.E. = +z$ (energy required to break the lattice). If $L.E.$ is given as $-z$ (energy released),then the energy to break the lattice is $+z$.Thus,$\Delta H_{sol} = z + (-x) + (-y) = z - (x + y)$.

The hydration energies of $K^{+}$ and $Cl^{-}$ are $-x$ and $-y$ $kJ / mol$ respectively. If the lattice energy of $KCl$ is $-z$ $kJ / mol$,then the heat of solution of $KCl$ is $:$

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