We’re being asked to calculate the value of the rate constant (k) based on the reaction and data given.

Recall that the **rate law** only focuses on the reactant concentrations and has a general form of:

$\overline{){\mathbf{rate}}{\mathbf{}}{\mathbf{law}}{\mathbf{=}}{\mathbf{k}}{\left[\mathbf{A}\right]}^{{\mathbf{x}}}{\left[\mathbf{B}\right]}^{{\mathbf{y}}}}$

k = rate constant

A & B = reactants

x & y = reactant orders

$\overline{){\mathbf{rate}}{\mathbf{}}{\mathbf{law}}{\mathbf{=}}{\mathbf{k}}{\mathbf{\left[}{\mathbf{OCl}}^{\mathbf{-}}\mathbf{\right]}}^{{\mathbf{x}}}{\mathbf{\left[}{\mathbf{I}}^{\mathbf{-}}\mathbf{\right]}}^{{\mathbf{y}}}{\mathbf{\left[}{\mathbf{OH}}^{\mathbf{-}}\mathbf{\right]}}^{{\mathbf{z}}}}$

**We’re going to calculate the rate law and the rate constant using the following steps:**

Consider this initial-rate data at a certain temperature for the reaction described by

Determine the rate law and the value of the rate constant for this reaction.

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