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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 (c) Calculate the time in half-lives when the inÂ­tegrated rate law is no longer valid, that is, when [A] t = 0.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 is \[r =2.0[A][B]^2\] The order of the reaction with respect to A is 1 and with respect to B is 2; the overall reaction order is as follows: 1 + 2 = 3. To calculate k, substitute the values from any one of the above trials into the rate law: 2.0 M/sec = k(1.00 M)(1.00M) 2 \[k = 2.0\; M^{-2}\; sec^{-1}\]