Concentration and Rate Law

The rate of a reaction often depends on the reactant concentrations. For any reaction, the relationship between the reaction rate and the reactant concentrations can be expressed mathematically using a rate law or the rate equation.

In a rate law, k is the proportionality constant, or the rate constant, and n is the reaction order with respect to a single reactant, whose value is often an integer. In rate laws for multi-reactant reactions, the overall reaction order is the sum of all reactant orders.

For each reactant, the reaction rate, rate constant, concentration, and the reaction order are all determined experimentally. The rate law expresses the relationship between all these parameters.

Individual reactant orders commonly take the values 0, 1, or 2, and based on the overall reaction order, chemical reactions can be categorized as zero-order, first-order, or second-order reactions.

A single-reactant, or unimolecular, chemical reaction for which the reaction rate remains constant throughout its duration is a zero-order reaction. The reactant order in a zero-order reaction is zero, and according to the rate law, the reactant concentration is raised to the zeroth power.

Since the