For the first part, we're being asked to determine the value of the rate constant.

For this, we will construct several graphs using the integrated rate law equations and select the graph that would generate a **straight line**

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

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

**y = mx + b**

where:

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

**Graph time vs. [A _{t}]**

A reaction in which A → products was monitored as a function of time and the results are shown below.

Determine the value of the rate constant.

What is the rate of reaction when [A] = 0.20 M?

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