Under which of the following conditions will a reaction be spontaneous when $\Delta$H^$\circ$ 0? A)"T$\Delta$S^$\circ$ = 0" B)"T$\Delta$S^$\circ$ $\Delta$H^$\circ$" C)"T$\Delta$S^$\circ$

Question

Under which of the following conditions will a reaction be spontaneous when $\Delta$H^$\circ$ > 0? A)"T$\Delta$S^$\circ$ = 0" B)"T$\Delta$S^$\circ$ > $\Delta$H^$\circ$" C)"T$\Delta$S^$\circ$ < 0^$\circ$" D)"$\Delta$G^$\circ$= 0"

Quizplus · Accepted Answer

According to the Gibbs free energy equation, a reaction is spontaneous if ΔG < 0. ΔG can be calculated using the equation ΔG = ΔH - TΔS, where ΔH is the change in enthalpy, ΔS is the change in entropy, and T is the temperature in Kelvin. In the provided equation, ΔG > 0. In order for ΔG to be less than 0, either ΔH must be negative or TΔS must be positive. Choice B states that the entropy change for the products is greater than the entropy change for the reactants, which would result in a positive value for TΔS. Therefore, B is the best choice as it provides a condition that would make the reaction spontaneous.

Under Which of the Following Conditions Will a Reaction Be Δ\DeltaΔ

Under Which of the Following Conditions Will a Reaction Be $\Delta$