The following reaction correctly shows the chemical equation for which the enthalpy of reaction is the lattice energy of KCl(s).KCl(s) $\rarr$K⁺(g) + Cl ^- (g)

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The reaction is correctly showing the chemical equation for the enthalpy of reaction as the lattice energy of KCl(s), which is represented by the initial reactant KCl(s) in the equation. The formation of gaseous K+ and Cl- ions from the solid KCl(s) requires energy input which is equal to the lattice energy of KCl, thus making this reaction endothermic.

The Following Reaction Correctly Shows the Chemical Equation for Which →\rarr→

The Following Reaction Correctly Shows the Chemical Equation for Which $\rarr$