CHM 112 Lecture Notes - Lecture 1: Arrhenius Equation, Linear Equation, Reaction Rate
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Rate = concentration / time m/s. Works for zero order and instantaneous reactions. Rate = final concentration - initial concentration / elapsed time. 4. initial rate (t=0 to t=any given time) Curved means that the rate changed and will reach equilibrium. Rate = k[a]^m + [b]^n + . Catalysis concentrations are part of a rate law. Law hold only at a given temperature. 1. calculate ln[a] and 1/[a] for all values. Whichever has the best straight line is the equation. The time required for [a]o to decrease by 50% Solve by plugging in [a]o=1 and [a]=0. 5 into rate equation. Half life is independent of initial reactant concentration. If you know t1/2 then you know k. Activation energy and temperature dependence of rate constants. 1. reacting molecules must encounter each other. High temperatures = fast molecules = more collisions. 1. increase concentrations of reactants - more molecules to collide. 2. increase temperature - molecules move faster.
