University College - Chemistry Chem 112A Lecture 31: Chemical Kinetics
5 Apr 2017
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Study the speed of reaction (reaction rates), the factors that influence them, and the mechanisms of reactions aa + bb -> cc + dd. Each time reaction occurs a of a and b of b are consumed, and c of c and d of d are produced. Rate of change of a over time = -d[a]/dt. Units for the rate of reaction: mol rxn/l/s. In general: rate of reaction = (cid:2869)(cid:3092)(cid:3293) (cid:3031)(cid:4670)(cid:3045)(cid:3032)(cid:3028)(cid:3030)(cid:3047)(cid:3028)(cid:3041)(cid:3047)(cid:3046)(cid:4671) (cid:3031)(cid:3047) Differential rate law how the rate of reaction is changing with respect to reactant conc. Rate = k[a]n[b]m n, m orders of reaction with respect to individual species. Only equal to the coefficients for elementary (single step) reactions. Units are dependent on the orders of reaction. Integrated rate law d[a]/[a] = -kdt (cid:1516) (cid:4670)(cid:3002)(cid:4671) (cid:4670)(cid:3002)(cid:4671)(cid:3116) (cid:3031)(cid:4670)(cid:3002)(cid:4671)(cid:3031)(cid:3047) = (cid:1516) (cid:1863)(cid:1856)(cid:1872) (cid:3047)(cid:2868) ln[a] ln[a]0 = -kt ln[a] = ln[a]0 kt. This is the integrated first order rate law.
