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a negative delta G (corresponding to a positive delta S) correlates to a spontaneous reaction, while a positive is vice versa. If the delta G is 0, the system will have reached equilibrium, and the forward and backward rates are the same.
A reaction will be spontaneous if the Gibbs free energy value is negative. So to find that point you would set the equation to zero to solve and then say that all values less that the one you find will make the reaction spontaneous.
When the change in Gibbs Free Energy value is negative, then we can know that the reaction is spontaneous and proceeding towards the products. If it is a positive change, then the reaction is not favorable or spontaneous and proceeds towards reactants.
A reaction is spontaneous if it has a negative delta G (meaning it also proceeds in the forward direction towards the products). When delta G is 0, the reaction is at equilibrium since the free energy of the products equals the free energy of the reactants and no more work can be done.
If DeltaG is less than 0 at a certain composition of the reaction mixture, then the forward reaction is spontaneous. If DeltaG is greater than 0 at a certain composition of the reaction mixture then the reverse reaction is spontaneous.
if delta G is less than 0, that means the reaction is spontaneous. You can also think of spontaneity in terms of the equation delta G= delta H - T*Delta S in order to assess which values of delta H and delta S can produce a spontaneous reaction with a negative delta G.
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