Consider the reaction of peroxydisulfate ion 1S2O82-2 with iodide ion 1I - 2 in aqueous solution: S2O8 2 - 1aq2 + 3 I - 1aq2¡2 SO42 - 1aq2 + I3- 1aq2 At a particular temperature, the initial rate of disappearance of S2O82 - varies with reactant concentrations in the following manner: Experiment 3S2o8 24 1M 2 3I4 1M 2 Initial Rate 1M,s2 1 0.018 0.036 2.6 * 10-6 2 0.027 0.036 3.9 * 10-6 3 0.036 0.054 7.8 * 10-6 4 0.050 0.072 1.4 * 10-5 (a) Determine the rate law for the reaction and state the units of the rate constant.

Key Concepts

Rate Law

The rate law expresses the relationship between the rate of a chemical reaction and the concentration of its reactants. It is typically formulated as Rate = k[A]^m[B]^n, where k is the rate constant, [A] and [B] are the concentrations of the reactants, and m and n are the reaction orders with respect to each reactant. Determining the rate law involves analyzing experimental data to find the values of m and n, which indicate how the rate is affected by changes in concentration.

Order of Reaction

The order of a reaction refers to the exponent to which the concentration of a reactant is raised in the rate law. It provides insight into the relationship between concentration and reaction rate. For example, a first-order reaction means that the rate is directly proportional to the concentration of that reactant, while a second-order reaction indicates that the rate is proportional to the square of the concentration. The overall order of the reaction is the sum of the individual orders.

Units of the Rate Constant (k)

The units of the rate constant (k) depend on the overall order of the reaction. For a zero-order reaction, the units are mol/L·s; for a first-order reaction, they are s^-1; and for a second-order reaction, they are L/(mol·s). Understanding the units of k is crucial for ensuring that the rate law is dimensionally consistent and for converting between different units in chemical kinetics.