Problem: The reaction A → B follows first order kinetics with k = 0.83 min–1. If the initial concentration of A is 3.6 M, what is the concentration of A after 15 minutes? A. 0.046 MB. 0.230 MC. 1.1×10–1 MD. 1.84×10–3 ME. 1.4×10–5 M

FREE Expert Solution

We’re given the following first order reaction:

A → B                 k = 0.83 min–1


The integrated rate law for a first order reaction is as follows:

ln[A]t = -kt + ln[A]0


where [A]t = concentration at time t, k = rate constant, t = time, [A]0 = initial concentration.


We’re being asked to calculate the amount of A after 15 mins if we start with 3.6 M A.


This means we have:

[A]0 = 3.6 M          k = 0.83 min–1

[A]t = ?                  t = 15 min


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Problem Details

The reaction A → B follows first order kinetics with k = 0.83 min–1. If the initial concentration of A is 3.6 M, what is the concentration of A after 15 minutes? 

A. 0.046 M

B. 0.230 M

C. 1.1×10–1 M

D. 1.84×10–3 M

E. 1.4×10–5 M

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