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Problem: Potassium perchlorate (KClO4) has a lattice energy of -599 kJ/mol and a heat of hydration of -548 kJ/mol.Determine the temperature change that occurs when 10.6 g of potassium perchlorate is dissolved with enough water to make 110.1 mL of solution. (Assume a heat capacity of 4.05 J/goC for the solution and a density of 1.05 g/mL.)

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We have to calculate the change in temperature that occurs when 10.6 g potassium perchlorate is dissolved to make 110.1 mL of solution.


Heat of solution is the energy absorbed or released when a solid is dissolved in a solvent to form a solution.

The heat of solution is calculated by this formula:

H°solution = H°hydration - H°lattice

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Problem Details

Potassium perchlorate (KClO4) has a lattice energy of -599 kJ/mol and a heat of hydration of -548 kJ/mol.

Determine the temperature change that occurs when 10.6 g of potassium perchlorate is dissolved with enough water to make 110.1 mL of solution. (Assume a heat capacity of 4.05 J/goC for the solution and a density of 1.05 g/mL.)

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Lattice Energy Application concept. If you need more Lattice Energy Application practice, you can also practice Lattice Energy Application practice problems.

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Based on our data, we think this problem is relevant for Professor Todd's class at VANDERBILT.