Given the following entropy values (in J K⁻¹ mol⁻¹) at 298 K and 1 atm: H2(g): 130.6, Cl2(g): 223.0, HCl(g): 186.7. The entropy change (in J K⁻¹ mol⁻¹) for the reaction H2(g) + Cl2(g) → 2HCl(g) is

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-166.9. The entropy change (ΔS) is calculated as the sum of the entropies of products minus the sum of the entropies of reactants. For the reaction: ΔS = [2 × S(HCl)] - [S(H2) + S(Cl2)] = [2 × 186.7] - [130.6 + 223.0] = 373.4 - 353.6 = -166.9 J K⁻¹ mol⁻¹.

Given the following entropy values (in J K⁻¹ mol⁻¹) at 298 K and 1 atm: H2(g): 130.6, Cl2(g): 223.0, HCl(g): 186.7. The entropy change (in J K⁻¹ mol⁻¹) for the reaction H2(g) + Cl2(g) → 2HCl(g) is

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