If $\Delta$_rG $\circ$ 0 for a reaction at all temperatures,then $\Delta$_rH $\circ$ is ____ and $\Delta$_rS $\circ$ is ____. A) negative,positive B) positive,negative C) negative,negative D) positive,positive E) positive,either positive or negative

Question

If $\Delta$_rG $\circ$ > 0 for a reaction at all temperatures,then $\Delta$_rH $\circ$ is ____ and $\Delta$_rS $\circ$ is ____. A) negative,positive B) positive,negative C) negative,negative D) positive,positive E) positive,either positive or negative

Quizplus · Accepted Answer

The given inequality shows that the reaction is exothermic (since the enthalpy change H is negative). As a result, the entropy change S must be negative for the reaction to be spontaneous at all temperatures (i.e. ΔG < 0). Therefore, F1F1F1S1F1F1F10_rSF1F1F1S1F1F1F10 must be negative, as the product side has lower entropy than the reactant side.

If Δ\DeltaΔ rG ∘\circ∘ > 0 for a Reaction at All Temperatures,then

If $\Delta$ _rG^$\circ$ > 0 for a Reaction at All Temperatures,then