The value of of anhydrous copper (II) sulphate is –66.11 kJ. Dissolution of 1 mole of blue vitriol, — Thermodynamics and Thermochemistry Chemistry Question
Question
The value of $\Delta H_{\text{sol}}$ of anhydrous copper (II) sulphate is –66.11 kJ. Dissolution of 1 mole of blue vitriol, [Copper (II) sulphate pentahydrate] is followed by absorption of 11.5 kJ of heat. The enthalpy of dehydration of blue vitriol is
Answer: B
💡 Solution & Explanation
$\text{CuSO}_4\text{(s)} \to \text{CuSO}_4\text{(aq)}$ ($\Delta H = -66.11\text{ kJ}$). $\text{CuSO}_4\cdot 5\text{H}_2\text{O(s)} \to \text{CuSO}_4\text{(aq)}$ ($\Delta H = +11.5\text{ kJ}$). The dehydration reaction is $\text{CuSO}_4\cdot 5\text{H}_2\text{O(s)} \to \text{CuSO}_4\text{(s)} + 5\text{H}_2\text{O(l)}$. $\Delta H = 11.5 - (-66.11) = +77.61\text{ kJ}$.
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