For a reaction to be spontaneous at any tempe | vedclass

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(A) For a reaction to be spontaneous,the Gibbs free energy change must be negative,i.e.,$\Delta G < 0$.According to the Gibbs-Helmholtz equation,$\Del

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$\Delta G < 0, \Delta H < 0$

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(A) For a reaction to be spontaneous,the Gibbs free energy change must be negative,i.e.,$\Delta G According to the Gibbs-Helmholtz equation,$\Delta G = \Delta H - T\Delta S$.For a reaction to be spontaneous at all temperatures,the enthalpy change $\Delta H$ must be negative (exothermic) and the entropy change $\Delta S$ must be positive.Thus,the condition is $\Delta G < 0$ and $\Delta H < 0$.

For a reaction to be spontaneous at any temperature,which of the following is true?

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