If $\Delta$G of a chemical reaction is negative and the change in entropy is positive, you can conclude that the reaction

Question

Quizplus · Accepted Answer

A negative ΔG indicates that the reaction is energetically favorable and can proceed spontaneously. A positive ΔS indicates that there is an increase in the disorder of the system. These two factors together suggest that the reaction is exergonic, meaning that it releases energy and proceeds spontaneously without an input of energy. Choice A is incorrect because the reaction doesn't require energy, and choice B is incorrect because an endergonic reaction absorbs energy from the surroundings rather than releasing it. Choice D is also incorrect as exergonic reactions reach equilibrium, and choice E is incorrect because the reaction increases the disorder in the system.

If Δ\DeltaΔ G of a Chemical Reaction Is Negative and the Change

If $\Delta$ G of a Chemical Reaction Is Negative and the Change