Question

Given the second law of thermodynamics and the mathematical definition of delta G, which reaction will be favorable: one with a decrease in free energy (deltaG<0) or one with an increase in free energy.

Answer 1

A reaction will be favorable when there is a decrease in free energy (delta G<0), which indicates a spontaneous and exergonic reaction.

Step-by-step explanation:

Given the second law of thermodynamics and the mathematical definition of delta G, a reaction with a decrease in free energy (delta G<0) will be favorable. This is because Gibbs free energy represents the usable energy in a system that is available to do work after accounting for entropy. When delta G is negative, indicating that the system is releasing energy, the reaction is considered exergonic and spontaneous in the forward direction, meaning it may occur without additional input of energy. Conversely, if delta G is positive, the reaction is non-spontaneous in the forward direction and may be spontaneous in the reverse direction.