Answer to Question #306704 in Biochemistry for Ali Hayes

Question

correct me if I am wrong:

when K is less than 1, the concentration of reactants is greater than products. Delta G is negative, or exergonic and K>Q, has a forward reaction

when K is greater than 1, the concentration of products is greater than reactants. Delta G is positive, or endergonic, and K<Q, has a reverse reaction.

I might have them wrong in some way, but this is why I am confused.

Also, is this correct for delta Gº:

if delta Gº is positive, there is a greater amount of reactants, a reverse reaction is favored to reach equilibrium. And if delta Gº is negative, there is a greater amount of products, and a forward reaction is favored to reach equilibrium.

Answer 1

when K is greater

than 1, the concentration of products is greater than reactants. Delta G is positive, or endergonic, and K.The products, or final state, have more free energy than the reactants, or initial state.

If delta Gº is positive,If ∆G° is positive at equilibrium, then we will have lots of reactants at equilibrium, meaning Q needs to be smaller (less than 1) to approach K. There is a greater amount of reactants, a reverse reaction is favored to reach equilibrium. And if delta Gº is negative, there is a greater amount of products, and a forward reaction is favored to reach equilibrium.