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Enthalpy of Solution

The table bel...

Question

The table below identifies three energy terms that must be considered in discussing the energy involved in forming aqueous solutions of solid ionic electrolytes.
Term Symbol
Lattice Energy of Solute $△ H_{l a t t i c e}$
Enthalpy of Solution $△ H_{s o l u t i o n}$
Enthalpy of Hydration $△ H_{h y d r a t i o n}$
Which of the following equation correctly expresses the relationship between the lattice energy of the solid solute, the enthalpy of solution, and the enthalpy of hydration of a solution of an electrolyte in water?

A

△ H_{s o l u t i o n} = △ H_{l a t t i c e} + △ H_{h y d r a t i o n}

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B

△ H_{h y d r a t i o n} = △ H_{s o l u t i o n} + △ H_{l a t t i c e}

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C

△ H_{l a t t i c e} = △ H_{s o l u t i o n} + △ H_{h y d r a t i o n}

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D

△ H_{s o l u t i o n} = △ H_{h y d r a t i o n} - △ H_{l a t t i c e}

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Solution

The correct option is B $△ H_{s o l u t i o n} = △ H_{l a t t i c e} + △ H_{h y d r a t i o n}$
${Δ H}_{h y d r a t i o n}$ is the enthalpy change when one mole of anhydrous substance undergoes complete combustion.
${Δ H}_{f u s i o n}$ is the enthalpy change that accompanies melting of one mole of solid substance.
${Δ H}_{s o l u t i o n}$ is the enthalpy change when one mole of a substance is dissolved in large excess of solvent, so that on further dilution no appreciable heat change occur.
So, ${Δ H}_{s o l u t i o n} = {Δ H}_{l a t t i c e} + {Δ H}_{h y d r a t i o n}$ .

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