CHM 2046 Lecture Notes - Lecture 2: Rate Equation, Reaction Rate Constant, Second Order (Religious)
18 Jan 2017
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The zero order integrated rate law is [at] [a0] = -kt, where: k = the rate constant, t = time in seconds. The first order integrated rate law is: ln[at] ln[a0] = -kt. This is proven by: rate = - [a]/ t and rate = k[a, k[a] = - [a]/ t. The second order integrated rate law is: 1/[at] 1/[a0] = kt. Example) the reaction a b has the rate law rate = k[a]2. In 10 minutes, the concentration of a drops from 1. 0m to 0. 5m. What is the rate constant for this reaction: 1/[at] 1/[a0] = kt, 1/[0. 5] 1/[1. 0] = k(600, k = 1. 7 x 10-3 or 0. 0017 m-1s-1. The units for a second order reaction will always be m-1s-1. Half life is the amount of time required for half of the amount of something to be used up: they are used to compare reactions of different orders. Zero order half life reactions: t1/2 = [a0]/2k.
