A reaction for which the change in Gibbs Free Energy is a negative value. Exothermic Spontaneous Endothermic Nonspontaneous
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Step 1: A negative change in Gibbs Free Energy indicates that the reaction is spontaneous. Show more…
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(A): All exothermic reactions are spontaneous at room temperature. $(\mathbf{R}):$ In $(\Delta \mathrm{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}), \Delta \mathrm{G}$ becomes negative and negative sign of $\Delta \mathrm{G}$ indicates spontaneous reaction.
The Gibbs energy change for a reaction is 298 kJ. The reaction is therefore: A. nonspontaneous B. exothermic C. equilibrium D. spontaneous
David C.
(A): Endothermic reaction is spontaneous at all temperatures. $(\mathbf{R}): \Delta \mathrm{G}$ is negative when $\mathrm{T} \Delta \mathrm{S}>\Delta \mathrm{H}$
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