No.
Change of Gibbs (free) energy:
- ∆G is the change of Gibbs (free) energy for a system and ∆G° is the Gibbs energy change for a system under standard conditions (1 atm, 298K).
- ∆G is the difference in the energy between reactants and products. In addition ∆G is unaffected by external factors that change the kinetics of the reaction.
- The value of ∆G and ∆G° differs leading to the change in the system.
→ If ∆G becomes equal to ∆G°, then ∆G° is not the free energy at equilibrium. When Gibbs free energy is zero, the reaction quotient becomes equilibrium constant.
Thus, the answer is No.
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