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

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

where:

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

**k** = rate constant

**t** = time, **[A] _{0}** = initial concentration.

The reactant concentration in a first-order reaction was 7.60×10^{−2} M after 35.0 s and 5.50×10^{−3} M after 85.0 s .

The reactant concentration in a first-order reaction was 7.60×10^{−2} M after 35.0 s and 5.50×10^{−3} M after 85.0 s .

What is the rate constant for this reaction?

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