For a given reaction,Delta H = 35.5 kJ mol^ | vedclass

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(A) The condition for spontaneity is $\Delta G < 0$.Given $\Delta G = \Delta H - T \Delta S$.For the reaction to be spontaneous,$\Delta H - T \Delta S

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$T > 425 \ K$

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(A) The condition for spontaneity is $\Delta G Given $\Delta G = \Delta H - T \Delta S$.For the reaction to be spontaneous,$\Delta H - T \Delta S  \Delta H$ or $T > \frac{\Delta H}{\Delta S}$.Given $\Delta H = 35.5 \ kJ \ mol^{-1} = 35500 \ J \ mol^{-1}$ and $\Delta S = 83.6 \ J \ K^{-1} \ mol^{-1}$.Calculating the equilibrium temperature: $T = \frac{35500}{83.6} \approx 424.64 \ K \approx 425 \ K$.Since $\Delta H > 0$ and $\Delta S > 0$,the reaction is spontaneous at temperatures higher than the equilibrium temperature,i.e.,$T > 425 \ K$.

For a given reaction,$\Delta H = 35.5 \ kJ \ mol^{-1}$ and $\Delta S = 83.6 \ J \ K^{-1} \ mol^{-1}$. The reaction is spontaneous at (Assume that $\Delta H$ and $\Delta S$ do not vary with temperature.)

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