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,

Which of the following represents the integrated rate law for a first-order reaction?

A) [A]_{t} - [A]_{0} = -kt

B) ln (k_{2}/k_{1}) = E_{a}/R(1/T) + lnA

C) ln ([A]_{t}/[A]_{0}) = -kt

D) k = A e(-E_{a}/RT)

E) 1/[A]_{t} - 1/[A]_{0} = kt

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