Which of the following is true for a spontaneous reaction at constant temperature? A) $\Delta$S + $\Delta$H/T

Question

Which of the following is true for a spontaneous reaction at constant temperature? A) $\Delta$S + $\Delta$H/T < 0 B) $\Delta$G° = 0 C) $\Delta$S_system < q/T D) $\Delta$H - T$\Delta$S < 0 E)$\Delta$S_surr > 0

Quizplus · Accepted Answer

For a spontaneous reaction at constant temperature, the change in Gibbs free energy (ΔG) must be negative. Using the equation ΔG = ΔH - TΔS, we can see that for a spontaneous reaction, ΔH must be negative and TΔS must be positive. Therefore, the correct answer is D, which states that ΔH and -TΔS are both negative, leading to a negative value for ΔG. The other answer choices do not provide accurate or relevant information to determine the spontaneity of the reaction at constant temperature.

Which of the Following Is True for a Spontaneous Reaction Δ\DeltaΔ

Which of the Following Is True for a Spontaneous Reaction $\Delta$