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

Consider the following elementary reaction equation.

H_{2}O_{2}(g) → H_{2}O(g) + O(g)

Rate Law:

$\overline{){\mathbf{Rate}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{k}}\mathbf{\left[}{\mathbf{H}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{2}}\mathbf{\right]}}$

*Concentrations are raised to power of each coefficient*

Consider the following elementary equation:

H_{2}O_{2}(g) → H_{2}O(g) + O(g)

What is the order with respect to H_{2}O_{2}?

What is the overall order of the reaction?

Classify the reaction as unimolecular, bimolecular, or termolecular.

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