1.How is the heat of solution of CaCl2 affected by: a) number of moles of CaCl2? b) number of moles of H2O?

Question

Explain the significance of the observation. In terms of partial molar volumes, lattice energy etc.

Answer 1

An increase in the number of moles of CaCl2 leads to a decrease in heat of solution because there is an increase in the number of bonds of CaCl2 to be broken, therefore more energy is absorbed in order to break the intermolecular bonds. An increase in the amount of H2O results in a decrease in the heat of solution because there are more molecules of water to absorb the heat produced. The reaction itself is endothermic, so there is less heat loss registered for the same amount of CaCl2 but with more water.

Answer 2

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Answer 3

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