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Asked by Pooja Last Modified
Answer At equilibrium, the Gibbs free energy change (ΔrGΔrG) will be zero. This is because at equilibrium, the forward and reverse reactions occur at the same rate, and there is no net change in the system.
The standard Gibbs free energy change (ΔrG∘ΔrG∘) is the Gibbs free energy change for a reaction under standard conditions (usually at 1 atm pressure and a specified temperature, often 298 K). ΔrG∘ΔrG∘ gives the Gibbs free energy change when all reactants and products are present at standard states (usually 1 M concentration for solutions).
While ΔrG∘ΔrG∘ provides important information about the thermodynamic feasibility of a reaction, it does not necessarily indicate whether a reaction is at equilibrium. Only when ΔrGΔrG is zero does it indicate that the reaction has reached equilibrium.
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