CHEM 116 Lecture Notes - Lecture 2: Rate Equation, Reaction Rate Constant, Activation Energy
Document Summary
Kinetics two molecules must collide with sufficient energy for a reaction of occur rate of reaction on the number of collisions/energy of collisions temperature: more molecules have more energy, so more reactive collisions. Catalyst: lowers the activation energy allowing more reactive collisions. Rate of change of species rate of production of products/loss of reactants. Average rate of production b = bt2-bt1/t2-t1 or b/ t. Average rate of loss a = at2-at1/t2-t1 or a/ t rate decreases with time instantaneous rate: rate at a particular time. Gain db/dt loss da/dt rate of reaction is the rate of production/loss of species rate of production/loss of species differs in the same reaction there is a unique number that gives the rate of reaction. Rate law for many chemical reactions the rate varies systematically with the concentration of the reaction this relationship is called the rate law. Many cases the rate law for aa + bb products can be written as rate = k[a]m[b]n.
