Given the following entropy values (in J/K-mol) at 298 K and 1 atm , and . The entropy change (in J/ — Thermodynamics and Thermochemistry Chemistry Question
Question
Given the following entropy values (in J/K-mol) at 298 K and 1 atm $\text{H}_2\text{(g)} = 130.6$, $\text{Cl}_2\text{(g)} = 223.0$ and $\text{HCl(g)} = 186.7$. The entropy change (in J/K-mol) for the reaction: $\text{H}_2\text{(g)} + \text{Cl}_2\text{(g)} \to 2\text{HCl(g)}$, is
Answer: D
💡 Solution & Explanation
$\Delta S^\circ_{rxn} = \sum S^\circ_{products} - \sum S^\circ_{reactants} = 2(186.7) - (130.6 + 223.0) = 373.4 - 353.6 = +19.8\text{ J/K-mol}$.
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