Find the bond energy of S–S bond from the following data:<br><br><br> — Thermodynamics and Thermochemistry Chemistry Question
Question
Find the bond energy of S–S bond from the following data:<br>$\text{C}_2\text{H}_5 - \text{S} - \text{C}_2\text{H}_5\text{(g)}; \Delta H_f^\circ = -148\text{ kJ}$<br>$\text{C}_2\text{H}_5 - \text{S} - \text{S} - \text{C}_2\text{H}_5\text{(g)}; \Delta H_f^\circ = -202\text{ kJ}$<br>$\text{S(g)}; \Delta H_f^\circ = 222\text{ kJ}$
Answer: A
💡 Solution & Explanation
Compare atomization energies to isolate the S-S bond. Atomization($\text{Et}_2\text{S}_2$) - Atomization($\text{Et}_2\text{S}$) equates strictly to $\text{BE(S-S)}$. Evaluating atomization differences via formation enthalpies gives: $[\Sigma \Delta H_f(\text{atoms}) - (-202)] - [\Sigma \Delta H_f(\text{atoms}) \text{ without 1 S} - (-148)] = \Delta H_f(\text{S, g}) + 202 - 148 = 222 + 54 = 276\text{ kJ/mol}$.
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