Why is Gibbs free energy zero at equilibrium?
Because at equilibrium, everything that
The Gibbs' free energy may have been given to you without really emphasizing that it is actually a function of temperature, pressure, and the
#\mathbf(G = G(T,P,n_1,n_2, . . . , n_N))#
When we are at equilibrium, we really mean all of the following are occurring:
- thermal equilibrium - the temperature is constant.
- pressure equilibrium - the pressure is constant.
- dynamic equilibrium - the concentration, and hence the
#"mol"#s, of reactants and products is steady/constant (but may react if disturbed).
But when all those things are constant, the Gibbs' free energy simply isn't changing at all. If the variables on which