Rate laws or rate equations are mathematical expressions that relate the rate of a chemical reaction to the concentrations of reactants (and sometimes products or catalysts). Often the rate of reaction is proportional to some power of the concentration of a substance involved in the reaction:

In the rate law, k is the rate constant, which is independent of concentrations. Each exponent, m, n, or p, defines the order of a reaction with respect to each reactant, A, B, or C. It is the power to which a concentration must be raised to correctly calculate the rate. For example, if m = 1, the reaction is first-order with respect to [A]; if n = 2, the reaction is second-order with respect to [B]; if p = 0, the reaction is zeroth-order with respect to [C], which means that the rate of the reaction is not affected by the concentration of C, because [C]⁰ = 1. The overall reaction order is the sum of the individual orders, m + n + p + … Reaction orders are usually positive integers, although they can be fractions or negative numbers.

Reaction Order and Rate Constant Units

It is often true that, as in the last activity, the reaction orders in the rate law are different from the coefficients in the chemical equation for the reaction. It is important to note that rate laws must be determined experimentally and are not reliably predicted by reaction stoichiometry.

Reaction orders play a role in determining the units for the rate constant—the units for k are whatever is needed so that substituting into the rate law expression affords the appropriate units for the rate.

The units for the rate constant for common reaction orders are summarized below.

Overall Reaction Order (m+n+…)	Units of k (M1-(m+n+…)s-1)
zeroth
first
second
third