Question

Which is more likely to be thermodynamically favored, the forward reaction or the reverse reaction?

Answer 1

Answer: The thermodynamic favorability of a chemical reaction can be determined by comparing the change in free energy (ΔG) between the reactants and products. A negative value of ΔG indicates that the reaction is thermodynamically favored, meaning that it is energetically favorable for the reaction to proceed in the forward direction. Conversely, a positive value of ΔG indicates that the reaction is not thermodynamically favored, and the reverse reaction is energetically favorable.

If the ΔG of the forward reaction is negative, the forward reaction will be thermodynamically favored, and the reverse reaction will not be. If the ΔG of the forward reaction is positive, the reverse reaction will be thermodynamically favored, and the forward reaction will not be. If the ΔG of the forward reaction is zero, the reaction is at equilibrium and neither the forward nor the reverse reaction is thermodynamically favored.

Therefore, whether the forward or reverse reaction is thermodynamically favored depends on the magnitude and sign of ΔG for that reaction.

Step-by-step explanation:

Answer 2

In chemistry, the likelihood of a reaction being thermodynamically favored depends on the change in Gibbs free energy, which is determined by both the enthalpy change and the entropy change of the reaction.

Step-by-step explanation:

In chemistry, the likelihood of a reaction being thermodynamically favored depends on the change in Gibbs free energy, which is determined by both the enthalpy change and the entropy change of the reaction.

If the forward reaction is thermodynamically favored, it means that the change in Gibbs free energy is negative (ΔG < 0) and the reaction is spontaneous in the forward direction. This means that the products are more stable than the reactants and the reaction will proceed in the forward direction without any additional energy input.

On the other hand, if the reverse reaction is thermodynamically favored, it means that the change in Gibbs free energy is positive (ΔG > 0) and the reaction is spontaneous in the reverse direction. This means that the reactants are more stable than the products and the reaction will proceed in the reverse direction without any additional energy input.