Problem: A → B is a first order reaction. Using the data below, what is the half-life in seconds? 0 sec, [A] = 1.22 M 3 sec, [A] = 0.86 M 6 sec, [A] = 0.61 M 9 sec, [A] = 0.43 M 12 sec, [A] = 0.31 M 15 sec, [A] = 0.22 M 18 sec, [A] = 0.15 M a. 2.3 sb. 2.8 sc. 6.1 sd. 7.8 se. 9.1 s

FREE Expert Solution

We are asked to determine the half-life of a 1st-order reaction using the provided data


The integrated rate law for a 1st-order reaction is as follows:


ln[N]t = -kt + ln[N]0


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

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Problem Details

A → B is a first order reaction. Using the data below, what is the half-life in seconds? 

0 sec, [A] = 1.22 M 

3 sec, [A] = 0.86 M 

6 sec, [A] = 0.61 M 

9 sec, [A] = 0.43 M 

12 sec, [A] = 0.31 M 

15 sec, [A] = 0.22 M 

18 sec, [A] = 0.15 M 

a. 2.3 s

b. 2.8 s

c. 6.1 s

d. 7.8 s

e. 9.1 s

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