If Δ_rG° 0 for a reaction at all temperatures,then Δ_rH° is _____ and Δ_rS° is _____. A) Negative; positive B) Positive; negative C) Negative; negative D) Positive; positive E) Positive; either positive or negative

Question

If Δ_rG° > 0 for a reaction at all temperatures,then Δ_rH° is _____ and Δ_rS° is _____. A) Negative; positive B) Positive; negative C) Negative; negative D) Positive; positive E) Positive; either positive or negative

Quizplus · Accepted Answer

If Δ_rG° > 0, then the reaction is spontaneous and Δ_rH° is positive, indicating that energy is absorbed by the reaction. This means that the products are less stable than the reactants. Furthermore, Δ_rS° is negative, indicating that the reaction leads to a decrease in disorder or an increase in order. The correct answer is therefore B, which has a positive Δ_rH° and a negative Δ_rS°.

If ΔrG° > 0 for a Reaction at All Temperatures,then

If Δ_rG° > 0 for a Reaction at All Temperatures,then