CHM 131 Lecture Notes - Lecture 7: Reaction Rate, Gibbs Free Energy, Ideal Gas

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Using lechatlier"s principle, we can see that if you add more to the reactants side of the reaction, the forward reaction will increase and the concentration of the products will be increased. The equilibrium constant depends on the ratio of the concentrations and remains the same. A large equilibrium constant doesn"t affect the rate of the reaction. The law of mass action states that the rate of a chemical reaction is proportional to the product of the reacting substance to the power of their corresponding coefficient. At equilibrium forward and backward rates are equal and the ratio of the rate constants is a constant and is known as an equilibrium constant. In a reaction mixture at equilibrium, the concentrations of the reactants and products are related by an equilibrium constant. Dd(g) + bb(g) cc(g) + aa(g) Forward reaction rate = backward reaction rate. The equilibrium constant is related to the standard gibbs free energy change for the reaction.

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