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:

$\overline{){\mathbf{ln}}{\mathbf{\left[}\mathbf{N}\mathbf{\right]}}_{{\mathbf{t}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{-}}{\mathbf{kt}}{\mathbf{}}{\mathbf{+}}{\mathbf{}}{\mathbf{ln}}{\mathbf{\left[}\mathbf{N}\mathbf{\right]}}_{{\mathbf{0}}}}$

where **[N] _{t}** = concentration at time t,

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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