Chlorine monoxide (ClO) decomposes at room temperature according to the reaction 2 ClO1g2¡Cl21g2 + O21g2 The concentration of ClO was monitored over time, and three graphs were made:

What is the rate law for the reaction? (LO 14.9) (a) Rate = k (b) Rate = k3ClO4 (c) Rate = k3ClO42 (d) Rate = k3ClO43 M14_MCMU6230_

The reaction order refers to the power to which the concentration of a reactant is raised in the rate law of a chemical reaction. It indicates how the rate of reaction depends on the concentration of reactants. For example, a first-order reaction means that the rate is directly proportional to the concentration of one reactant, while a second-order reaction involves the square of the concentration. Understanding the reaction order is crucial for determining the rate law.

The rate law is an equation that relates the rate of a chemical reaction to the concentration of its reactants. It is typically expressed in the form Rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to reactants A and B, respectively. The rate law provides insight into the mechanism of the reaction and is determined experimentally, often through concentration vs. time data.

First-order reactions are characterized by a linear relationship between the natural logarithm of the concentration of a reactant and time. This means that as the concentration decreases, the rate of reaction remains proportional to the concentration of the reactant. The provided graph of the natural logarithm of ClO concentration over time indicates a straight line, confirming that the decomposition of ClO follows first-order kinetics, which is essential for determining the correct rate law.