At a particular temperature and [A]0 = 2.00 x 10-2 concentration versus time data were collected for this reaction, and a plot of 1/[A] versus time resulted in a straight line with a slope value of -2.97 x 10-2 min-1(a) Determine the rate law, the intergrated rate law, and the value of the rate constant for this reaction.
Rate law
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Rate = k[A]3
The equation described in your answer is not balanced.
Integrated rate law
1/[A] = kt + 1/[A]0
1/[B] = kt + 1/[B]0
[A]/kt = [B]
kt = [A]/[B]
(b) Calculate the half-life for this reaction.
(c) How much time is required for the concentration of A to decrease to 2.50 x 10-3 M?