For the spontaneity of a reaction,which state | vedclass

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

Vedclass · Accepted Answer

$\Delta H = - ve$; $\Delta S = + ve$

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(D) The spontaneity of a reaction is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T\Delta S$. For a reaction to be spontaneous,$\Delta G$ must be negative $(\Delta G If $\Delta H$ is negative (exothermic) and $\Delta S$ is positive (increase in entropy),then $\Delta G = (	ext{negative}) - T(	ext{positive})$. Since $T$ (absolute temperature) is always positive,$-T\Delta S$ will be negative. Therefore,$\Delta G$ will always be negative regardless of the temperature,making the reaction always spontaneous.

For the spontaneity of a reaction,which statement is always true?

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