CHEM 120 Lecture Notes - Lecture 8: Intermediate Consumption, Reversible Reaction, Equilibrium Constant

• School: McGill University
• Department: Chemistry
• Course: CHEM 120
• Professor: Laura Pavelka, Samuel Sewall, Pallavi Sirjoosingh

Document Summary

The concentration of the intermediates remains constant through the reaction. Production of intermediate = consumption of intermediate. Can change number of steps in a reaction or maintain the same number of steps but just decrease ea. Catalysts is in the same phase as the reactants. Absorption on the surface of the catalyst. Catalytic surface provides an active site for the reaction. D[es]/dt = k1[e][s] - k-1[es] - k2[es] 0 = k1[e][s] - k-1[es] - k2[es] K1([e]0 - [es])[s] = (k-1 + k2)[es] Reversible reaction do not have to have the same ea in eh forward and reverse directions. After a certain period of time, concentrations of reactants/products no longer change. At equilibrium, two opposing processes take place at equal rates ratefwd=raterev.