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The integrated rate law for the zero-order reaction A âB is [A] t = [A] 0 â kt. (a) Sketch the following plots: (i) rate versus [A] t and. (ii) [A] t versus t. (b) Derive an expression for the half-life of the reacÂ­tion. (c) Calculate the time in half-lives when the inÂ­tegrated rate law is no longer valid, that is, when [A] t = 0. STEP-BY-STEP SOLUTION. JavaScript Not Detected. JavaScript is required to view textbook solutions.
Therefore, the rate law for this reaction is: rate = k[NO] 2 [O 2 ]. This reaction is second order in nitric oxide, and first order in oxygen. It is third order overall. The fact that the reaction is first order in O 2 means that the rate is directly proportional to the O 2 concentration.If [O 2 ] doubles or triples, the rate will double or triple also. We can show this mathematically. Consider two experiments.he fact that the reaction is first order in O 2 means that the rate is directly proportional to the O 2 concentration. If [O 2 ] doubles or triples, the rate will double or triple also. We can show this mathematically.