For a reaction at standard conditions, if ΔG° is positive, what does it indicate

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Question: For a reaction at standard conditions, if ΔG° is positive, what does it indicate?

Options:

Correct Answer: The reaction is non-spontaneous in the forward direction.

Solution:

A positive ΔG° indicates that the reaction is non-spontaneous in the forward direction.

For a reaction at standard conditions, if ΔG° is positive, what does it indicate?

For a reaction at standard conditions, if ΔG° is positive, what does it indicate?

Step 1: Understand what ΔG° means. ΔG° is the change in Gibbs free energy for a reaction at standard conditions.
Step 2: Recognize that a positive ΔG° value indicates that the energy of the products is higher than the energy of the reactants.
Step 3: Know that if a reaction has a positive ΔG°, it means that the reaction does not occur spontaneously in the forward direction.
Step 4: Conclude that a positive ΔG° suggests that the reaction will require energy input to proceed.

Gibbs Free Energy – Gibbs Free Energy (ΔG) is a thermodynamic potential that indicates the spontaneity of a reaction; a positive ΔG° means the reaction is non-spontaneous under standard conditions.
Spontaneity of Reactions – A reaction is spontaneous if it can occur without external intervention; a positive ΔG° suggests that the reaction will not proceed in the forward direction without additional energy input.