For the second-order reaction A → products, the following data are obtained: [A] = 3.024 M, t = 0 min
[A] = 2.935 M, t = 1.0 min
[A] = 2.852 M, t = 2.0 min
What is the concentration of [A] after 4 min?

Question

Quizplus · Accepted Answer

The rate law for a second-order reaction is:rate = k[A]^2where k is the rate constant and [A] is the concentration of the reactant.We can use the integrated rate law to determine the concentration of [A] at any time t:1/[A] = kt + 1/[A]0where [A]0 is the initial concentration of [A].We can use the data given in the question to determine the value of k:1/2.935 - 1/3.024 = k(1.0 - 0)k = 0.089 M^-1 min^-1Now we can use the integrated rate law to determine the concentration of [A] after 4 min:1/[A] = 0.089 M^-1 min^-1 * 4 min + 1/3.024 M[A] = 2.70 MTherefore, the correct answer is A) 2.70 M.

For the Second-Order Reaction a → Products, the Following Data