The standard reaction Gibbs energy for a chem | vedclass

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Question

(A) The standard Gibbs energy equation is given by $\Delta G^{o} = \Delta H^{o} - T\Delta S^{o}$.Comparing this with the given equation $\Delta G^{o}

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Endothermic if $A > 0$

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(A) The standard Gibbs energy equation is given by $\Delta G^{o} = \Delta H^{o} - T\Delta S^{o}$.Comparing this with the given equation $\Delta G^{o} = A - BT$,we find that $A = \Delta H^{o}$ and $B = \Delta S^{o}$.For an endothermic reaction,the enthalpy change $\Delta H^{o}$ is positive,which implies $A > 0$.For an exothermic reaction,the enthalpy change $\Delta H^{o}$ is negative,which implies $A Therefore,the reaction is endothermic if $A > 0$.

The standard reaction Gibbs energy for a chemical reaction at an absolute temperature $T$ is given by $\Delta_{r}G^{o} = A - BT$,where $A$ and $B$ are non-$zero$ constants. Which of the following is $TRUE$ about this reaction?

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