CHEM 122 Chapter : 15.4 The Integrated Rate Law.docx
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13 Dec 2012
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Expressing the rate as a function of time. Formed from the given differential rate law. If reaction is in first order, rate = -d[n2o5]/dt = k[n2o5] Integrated rate law: ln[n2o5] = -kt + ln[n2o5]o. The equation shows how [a] depends on time. If [a]o and value of the rate constant, k, are known, the concentration of a at any time can be calculated. Y = mx + b; y = ln[a] x = t m = -k b = ln[a]o. Reaction is in first order if a plot of ln[a] vs. time gives a straight line. The integrated rate law can also be represented in terms of the ratio of [a] and. Time required for a reactant to reach half its original concentration t1/2 = 0. 693/k *half-life does not depend on initial concentration. If the reaction is second order, rate = -d[a]/dt = k[a]2. Integrated rate law: 1/[a] = kt + 1/[a]o.
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