Final answer:
The standard Gibbs free energy is zero at equilibrium. It is never zero in a closed system.
Step-by-step explanation:
The standard Gibbs free energy is zero at a specific condition known as equilibrium. This means that there is no net change in the concentration of reactants and products because the forward and reverse reactions occur at the same rate.
It is important to recognize that standard Gibbs free energy being zero is an indicator of equilibrium but not of the spontaneity or direction of a reaction at temperatures apart from the standard conditions.
For a reaction at a given temperature, if the Gibbs free energy change (ΔG) is zero, the system is at equilibrium. A spontaneous process occurs when ΔG is negative, while a non-spontaneous process would have a positive ΔG. The value of ΔG is dependent on the reaction conditions, including temperature, pressure, and the specific states of the reactants and products involved.
The Gibbs free energy (G) is a thermodynamic function that can be used to predict the spontaneity of a reaction. At equilibrium, the standard Gibbs free energy is zero, indicating that the system is in a state of balance. This means that the forward and reverse reactions are occurring at the same rate
In a closed system, the standard Gibbs free energy may not always be zero. It depends on the conditions of the reaction. At high temperatures, the standard Gibbs free energy can be negative, indicating that the reaction is spontaneous. However, it is important to note that the standard Gibbs free energy is never zero in a closed system.