The tabulated data were collected for this reaction: 2 NO2(g) + F2(g) → 2 NO2F(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

insert step 1: Identify the general form of the rate law for the reaction. The rate law is typically expressed as: rate = k [NO_2]^m [F_2]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to NO_2 and F_2, respectively.

insert step 2: Use the experimental data to determine the reaction orders m and n. This is done by comparing the changes in concentration and the corresponding changes in the reaction rate.

insert step 3: Once the reaction orders m and n are determined, substitute them back into the rate law expression.

insert step 4: Use the experimental data to calculate the rate constant k. Choose one set of experimental data, substitute the concentrations and the rate into the rate law, and solve for k.

insert step 5: Determine the overall order of the reaction by adding the reaction orders m and n. The overall order is the sum of the exponents in the rate law expression.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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. Understanding how to derive the rate law from experimental data is crucial for analyzing reaction kinetics.

Rate Constant (k)

The rate constant, k, is a proportionality factor in the rate law that is specific to a given reaction at a particular temperature. It reflects the speed of the reaction and can be influenced by factors such as temperature and the presence of catalysts. Calculating k involves using experimental data to determine the rate of reaction and the concentrations of reactants at that rate.

Overall Order of Reaction

The overall order of a reaction is the sum of the powers of the concentration terms in the rate law. It provides insight into the relationship between reactant concentrations and the rate of reaction. For example, if the rate law is rate = k[NO2]^1[F2]^1, the overall order would be 2, indicating that the reaction rate depends on the concentrations of both reactants.

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Related Practice

Textbook Question

A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. a. Write a rate law for the reaction.

Textbook Question

A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)? d. By what factor does the reaction rate change if [B] is doubled? e. By what factor does the reaction rate change if [C] is doubled? f. By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)?

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Textbook Question

Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A. What is the order of the reaction? Write a rate law for the reaction including the value of the rate constant, k.

Textbook Question

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?

Textbook Question

Indicate the order of reaction consistent with each observation.

a. The half-life of the reaction gets shorter as the initial concentration is increased.

b. A plot of the natural log of the concentration of the reactant versus time yields a straight line.

Textbook Question

Indicate the order of reaction consistent with each observation c. The half-life of the reaction gets longer as the initial concentration is increased.