Under what conditions will a reaction become | vedclass

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(B) 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

$\Delta H = -ve, \quad \Delta S = +ve$

Vedclass · Answer

(B) 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 at all temperatures,$\Delta G$ must be negative at all values of $T$. If $\Delta H$ is negative (exothermic) and $\Delta S$ is positive (increase in entropy),then $\Delta G = (	ext{negative}) - T(	ext{positive})$. Since $T$ is always positive in Kelvin,$-T\Delta S$ will always be negative. Thus,$\Delta G$ will always be negative regardless of the temperature.

Under what conditions will a reaction become spontaneous at all temperatures?

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