K = 1 ln 1 = 0
0 < K < 1 ln K = negative (–) value
K > 1 ln K = positive (+) value
ln 1 = 0 ΔG°rxn = 0
ln K = negative (–) value ΔG°rxn = positive (+) value → reactant-favored
ln K = positive (+) value ΔG°rxn = negative (–) value → product-favored
Filling in the blanks:
If the value of the equilibrium constant, K, for a reaction is greater than 1, the value of ΔG for the reaction is________- and the reaction is___________ .
If the value of K for a reaction is less than 1 the value of ΔG for the reaction is________ and the reaction is________ .
(hint: the value for ΔG will either be "positive" or "negative." Type in the proper word. Do not use quotations marks or "+" or "-" in your answer. The reaction will be "product-favored" or "reactant-favored." Type in the appropriate response, including the hyphen. To be sure you understand: To say a reaction is product-favored means the forward reaction is spontaneous, the reverse reaction is nonspontaneous, and the equilibrium mixture will contains greater concentrations of products than reactants. Spontaneous reactions are those that result in a lower total Gibbs free energy of the system. To say a reaction is nonspontaneous does not mean it cannot happen. It means energy must be added to the system to make it happen. To say a reaction is reactant-favored means the reverse reaction is spontaneous, the forward reaction is nonspontaneous, and the equilibrium mixture will contains greater concentrations of reactants than products.