Recall that each** straight line plot** (A = concentration of reactant) corresponds to:

**[A] vs. time (in s) →****Zeroth-order reaction****ln[A] vs. time (in s) →****First-order reaction****1/[A] vs. time (in s) →****Second-order reaction**

*Integrated rate law:*

- Zeroth order reaction:

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

- First-order reaction:

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

- Second-order reaction is as follows:

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

Assuming, X = reactant and Y = product:

**Reaction: X → Y**

Identify what the graphs of [X] versus time and [Y] versus time would look like for various orders.

Zero-order [X] vs. t

Zero-order [Y] vs. t

First or Second-order [X] vs. t

First or Second-order [Y] vs. t

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