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

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

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 a reaction is considered spontaneous if it can occur without external energy input.
Step 4: Since ΔG° is positive, it means the reaction does not occur naturally in the forward direction under standard conditions.
Step 5: Conclude that a positive ΔG° implies the reaction is non-spontaneous in the forward direction.

Gibbs Free Energy – ΔG° represents the change in Gibbs free energy for a reaction at standard conditions, indicating the spontaneity of the reaction.
Spontaneity of Reactions – A positive ΔG° means the reaction does not occur spontaneously in the forward direction, implying that the reactants are favored over the products.