We’re being asked to calculate the value of the rate constant (in L/min•mol) for the reaction below if the reaction is 20.0 =% complete in 26.2%.

**A → B + C**

The ** integrated rate law** for a second-order reaction is as follows:

$\overline{)\frac{\mathbf{1}}{{\mathbf{\left[}\mathbf{A}\mathbf{\right]}}_{\mathbf{t}}}{\mathbf{=}}{\mathbf{kt}}{\mathbf{+}}\frac{\mathbf{1}}{{\mathbf{\left[}\mathbf{A}\mathbf{\right]}}_{\mathbf{0}}}}$

where:

**[A] _{t}** = concentration at time t

**k** = rate constant

**t** = time (unknown)

**[A] _{0}** = initial concentration

The reaction A => B + C is second order in A. When the initial [A] = 0.100 M, the reaction is 20.0% complete in 26.2 minutes. Calculate the value of the rate constant (in L/min·mol).

A. 6.54x10^{-2}

B. 9.54x10^{-5}

C. 1.52

D. 9.54x10^{-2}

E. 4.40

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