16.34 g of cuso4 dissolved in water giving out 55.51 kj and 25.17 g cuso4•5h2o absorbs 95.31 kj. from the following reaction cycle and the experimental data above, calculate the enthalpy of hydration of cuso4.

The enthalpy of hydration of copper sulphate is -1486.62 kJ/mol which means 1486.62kJ of energy is absorbed by one mole of copper sulphate during the process of hydration

Explanation:

Step 1: Determine the energy released per mole of dissolved

(Eq. 1)

If 0.102 moles of releases 55.51kJ of energy, 1 mole will release 541.85kJ/mol

ΔH = -541.85kJ/mol

Step 2: Determine the energy released per mole of dissolved

(Eq. 2)

If 0.101 moles of absorbs 95.31kJ of energy, 1 mole will absorb 944.77kJ/mol

ΔH = 944.77kJ/mol

Step 3: Subtracting Eq. 2 from Eq. 1

ΔH = -541.85kJ/mol (Eq. 1)

ΔH = 944.77kJ/mol (Eq. 2)

ΔH = -541.85-944.77

ΔH = -1486.62 kJ/mol

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