The first-order decomposition, A $\rarr$ products, has a rate constant of 0.150 s^-1. Starting with [A]_o = 0.350 M, how much time is required for [A]_t = 0.125 M

Question

Quizplus · Accepted Answer

Explanation:The integrated rate law for a first-order reaction is:ln([A]t/[A]o) = -ktwhere [A]t is the concentration of A at time t, [A]o is the initial concentration of A, k is the rate constant, and t is time.We can use this equation to solve for t:t = -ln([A]t/[A]o)/kPlugging in the given values, we get:t = -ln(0.125/0.350)/0.150 s^-1 = 6.86 sTherefore, the correct answer is A.

The First-Order Decomposition, A →\rarr→ Products, Has a Rate Constant of 0

The First-Order Decomposition, A $\rarr$ Products, Has a Rate Constant of 0