The tabulated data were collected for this reaction: CH₃Cl(g) + 3 Cl₂(g) → CCl₄( g) + 3 HCl(g)

Write an expression for the reaction rate law and calculate the value of the rate constant, k. What is the overall order of the reaction?

Verified step by step guidance

1. Identify the general form of the rate law for the reaction: rate = k[A]^m[B]^n.
2. Use the data from the table to set up ratios of the rates and concentrations to determine the reaction orders m and n.
3. Compare experiments 1 and 2 where [B] is constant to find the order with respect to [A].
4. Compare experiments 1 and 3 where [A] is constant to find the order with respect to [B].
5. Once the orders m and n are determined, use any set of data from the table to solve for the rate constant k.

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.

Order of Reaction

The order of a reaction is the sum of the exponents in the rate law expression. It indicates how the rate of reaction is affected by the concentration of the reactants. A reaction can be zero, first, second, or higher order, depending on the values of m and n. Understanding the order helps predict how changes in concentration will influence the reaction rate.

Rate Constant (k)

The rate constant, k, is a proportionality factor in the rate law that is specific to a particular reaction at a given temperature. It reflects the speed of the reaction and is influenced by factors such as temperature and the presence of catalysts. To calculate k, one can rearrange the rate law using known concentrations and initial rates from experimental data.