The spontaneous nature of a reaction is impos | vedclass

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Question

(D) The spontaneity of a reaction is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T \Delta S$.$A$ reaction is spontaneous if $

Vedclass · Accepted Answer

$\Delta H$ is $+ve$; $\Delta S$ is negative

Vedclass · Answer

(D) The spontaneity of a reaction is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T \Delta S$.$A$ reaction is spontaneous if $\Delta G If $\Delta H$ is $+ve$ (endothermic) and $\Delta S$ is $-ve$ (decrease in entropy),then $\Delta G = (+ve) - T(-ve) = (+ve) + T(+ve)$,which results in a positive $\Delta G$ at all temperatures.Therefore,the reaction is non-spontaneous (impossible) under these conditions.

The spontaneous nature of a reaction is impossible if

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