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measures how much potential a reaction has left to do a net amount of something. If is negative, the forward reaction is favored. If is positive, the reaction is reactant favored. If the free energy is zero, the reaction is at equilibrium because there is no more net work to be done. This means the reaction is not spontaneous in either direction.
When Delta =0 it means that neither the formation of products nor reactants will be favored. This relates to our previous understanding of equilibrium from Chem 14 A where we understood that at equilibrium the rate of creation of products and reactants will be stable.
Delta G refers to the spontaneity of a reaction, so if delta G is positive, then the reaction is not spontaneous and the reactants are favored, but when it is negative, the reaction is spontaneous and the products are favored. So, when delta G is 0 neither the products nor reactants are favored thus the reaction is at equilibrium
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