What does a ΔG value of zero indicate about a reaction?

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Question: What does a ΔG value of zero indicate about a reaction?

Options:

Correct Answer: The reaction is at equilibrium.

Solution:

A ΔG value of zero indicates that the reaction is at equilibrium, meaning the forward and reverse reactions occur at the same rate.

What does a ΔG value of zero indicate about a reaction?

What does a ΔG value of zero indicate about a reaction?

Step 1: Understand what ΔG means. ΔG stands for Gibbs free energy change, which tells us about the energy available for a reaction to do work.
Step 2: Know that a ΔG value can be positive, negative, or zero. A positive ΔG means the reaction needs energy to occur, a negative ΔG means the reaction releases energy, and a zero ΔG means something different.
Step 3: Recognize that a ΔG value of zero indicates that the reaction is at equilibrium. This means that the rate of the forward reaction (reactants turning into products) is equal to the rate of the reverse reaction (products turning back into reactants).
Step 4: Conclude that at equilibrium, the concentrations of reactants and products remain constant over time, even though both reactions are still happening.

Gibbs Free Energy (ΔG) – ΔG is a thermodynamic potential that indicates the spontaneity of a reaction; a value of zero signifies equilibrium.
Chemical Equilibrium – At equilibrium, the rates of the forward and reverse reactions are equal, leading to no net change in the concentrations of reactants and products.