Explanation Step 1: In order to form the solution, the molecules of the solvent must move apart to accommodate the solute molecules. Since the solvent molecule attracts each other, energy must be expanded to separate them and the enthalpy change is endothermic (ΔH 1 ) . Step 2: The solute molecule must be separated from each other to enter the solution, and the enthalpy change is endothermic (ΔH 2 ) . Step 3: When solvent is added to a solution, steps one and two are both endothermic because the energy is required to overcome the intermolecular interactions in the solvent and in the solute. Since the enthalpy is positive for both steps 1 and 2, the solute-solvent interactions (ΔH 3 ) must be stronger than the solute-solute interactions and solvent-solvent interactions they replace in order for the dissolution process to be exothermic. (ΔH soln <0)

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ISBN: 9780534420123

Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher: Cengage Learning

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Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to a…

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Chapter 12, Problem 12.4QE

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Interpretation:

The relative enthalpy changes of the three listed processes have to be given.

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Chapter 12, Problem 12.3QE

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Chemistry: Principles and Practice

Ch. 12 - Prob. 12.1QE Ch. 12 - Prob. 12.2QE Ch. 12 - Prob. 12.3QE Ch. 12 - Prob. 12.4QE Ch. 12 - Prob. 12.5QE Ch. 12 - Prob. 12.6QE Ch. 12 - Prob. 12.7QE Ch. 12 - Prob. 12.8QE Ch. 12 - Prob. 12.9QE Ch. 12 - Prob. 12.10QE

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