Standard entropies for H_2, Cl_2 and HCl are | vedclass

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(C) The expression for entropy change is $\Delta S = \sum [n 	imes S_{	ext{product}}] - \sum [n 	imes S_{	ext{reactant}}]$.For the reaction $H_2 +

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$1500$

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(C) The expression for entropy change is $\Delta S = \sum [n 	imes S_{	ext{product}}] - \sum [n 	imes S_{	ext{reactant}}]$.For the reaction $H_2 + Cl_2 ightleftharpoons 2HCl$:$\Delta S = [2 	imes 60] - [1 	imes 60 + 1 	imes 40] = 120 - 100 = 20 \ J \ K^{-1}$.At equilibrium,the Gibbs free energy change $\Delta G = 0$.Since $\Delta G = \Delta H - T \Delta S$,at equilibrium,$\Delta H = T \Delta S$.Given $\Delta H = +30 \ kJ = 30000 \ J$ and $\Delta S = 20 \ J \ K^{-1}$.$30000 \ J = T 	imes 20 \ J \ K^{-1}$.$T = \frac{30000}{20} = 1500 \ K$.

Standard entropies for $H_2, Cl_2$ and $HCl$ are $60, 40$ and $60 \ J \ K^{-1} \ mol^{-1}$ respectively. For the reaction $H_2 + Cl_2 \rightleftharpoons 2HCl$,with $\Delta H = +30 \ kJ$,the temperature at which the reaction will be at equilibrium is $..... \ K$.

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