What is the relationship between ΔH and ΔG at equilibrium?

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Question: What is the relationship between ΔH and ΔG at equilibrium?

Options:

Correct Answer: ΔG = 0

Solution:

At equilibrium, the change in Gibbs free energy (ΔG) is zero.

What is the relationship between ΔH and ΔG at equilibrium?

What is the relationship between ΔH and ΔG at equilibrium?

Step 1: Understand that ΔH represents the change in enthalpy, which is the total heat content of a system.
Step 2: Understand that ΔG represents the change in Gibbs free energy, which indicates the spontaneity of a reaction.
Step 3: Know that at equilibrium, a chemical reaction has reached a state where the forward and reverse reactions occur at the same rate.
Step 4: Recognize that at equilibrium, there is no net change in the concentrations of reactants and products.
Step 5: Realize that when a system is at equilibrium, the change in Gibbs free energy (ΔG) is zero, meaning the system is stable.

No concepts available.