Question

The overall enthalpy change during the process of forming a solution involves three terms: separating solvent...

The overall enthalpy change during the process of forming a solution involves three terms: separating solvent molecules (ΔH°solvent), separating solute particles (ΔH°solute), and forming new solute-solvent associations (ΔH°solution). The overall process of forming a solution is endothermic if

a. IΔH°solute + ΔH°solventI > IΔH°solutionI

b. IΔH°solute + ΔH°solventI = IΔH°solutionI

c. IΔH°solute + ΔH°solventI < IΔH°solutionI

d. ΔH°solute + ΔH°solvent = 0

e. ΔH°solution = 0

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Homework Answers

Answer #1

The overall enthalpy change in the formation of the solution (ΔHsoln) is the sum of the enthalpy changes in the three steps:

ΔHsoln=ΔH1+ΔH2+ΔH3

When a solvent is added to a solution, steps 1 and 2 are both endothermic because energy is required to overcome the intermolecular interactions in the solvent (ΔH1) and the solute (ΔH2). Because ΔH is positive for both steps 1 and 2, the solute–solvent interactions (ΔH3) must be stronger than the solute–solute and solvent–solvent interactions in order a process to be exothermic (ΔHsoln<0). If (ΔHsoln>0) then it is endothermic.

Therefore answer is A i.e., IΔH°solute + ΔH°solventI > IΔH°solutionI

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