In chapter 4 of the chemistry content review;
When discussing Enthalpy, it made perfect sense that when Keq = Q , the system is in equilibrium. However, when discussing Gibbs Free Energy, it made it appear that equilibrium occurs when Keq = 1. Don't these two principles conflict, for Keq doesn't have to be 1 for the system to be at equilibrium right?
The book is correct. Equilibrium, in a chemical sense, represents that the formation of reactants and products has reached a balance where the rate of forward reaction is equal to the reverse reaction. This is represented by a Keq of 1, meaning that the products and reactants have reached a balance between the two. A Keq greater than 1 would symbolize a reaction that is favoring the products, while a Keq of less than 1 would show a reaction that is favoring the reactants.