The enthalpy change for the reaction, is –57 kJ. Predict the value of the enthalpy change in the fol — Thermodynamics and Thermochemistry Chemistry Question
Question
The enthalpy change for the reaction, $\text{NaOH(aq)} + \text{HCl(aq)} \to \text{NaCl(aq)} + \text{H}_2\text{O(l)}$ is –57 kJ. Predict the value of the enthalpy change in the following reaction:<br>$\text{Ba(OH)}_2\text{(aq)} + \text{H}_2\text{SO}_4\text{(aq)} \to \text{BaSO}_4\text{(s)} + 2\text{H}_2\text{O(l)}$
Answer: D
💡 Solution & Explanation
The target reaction involves the neutralization of 2 moles of $\text{H}^+$ and $\text{OH}^-$, providing $2 \times (-57) = -114\text{ kJ}$. Additionally, the precipitation of the insoluble $\text{BaSO}_4\text{(s)}$ releases further lattice/precipitation energy. Thus, the total energy released must be significantly more exothermic than -114 kJ, matching strictly with -200 kJ.
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