A proposed mechanism for the oxidation of nitric oxide to nitrogen dioxide was described in Problem 14.29. Another possible mechanism for this reaction is
(c) Relate the rate constant k to the rate constants for the elementary reactions.

Verified step by step guidance

1. Identify the elementary reactions involved in the proposed mechanism.
2. Write the rate law for each elementary step based on its molecularity.
3. Determine the rate-determining step (RDS) of the mechanism, which is the slowest step.
4. Express the overall rate law in terms of the rate constant k and the rate constants of the elementary reactions.
5. Relate the rate constant k of the overall reaction to the rate constants of the elementary steps, considering the RDS and any fast equilibrium steps.

Key Concepts

Rate Constant (k)

The rate constant (k) is a proportionality factor in the rate law of a chemical reaction, indicating the speed at which the reaction occurs. It is specific to a particular reaction at a given temperature and is influenced by factors such as concentration and activation energy. Understanding k is essential for relating the overall reaction rate to the concentrations of reactants.

Elementary Reactions

Elementary reactions are single-step processes that describe the direct transformation of reactants into products. Each elementary reaction has its own rate constant, which contributes to the overall rate of a complex reaction mechanism. Analyzing these steps helps in understanding how the overall reaction rate can be derived from the individual steps.

Reaction Mechanism

A reaction mechanism is a detailed description of the step-by-step sequence of elementary reactions that lead to the overall transformation of reactants into products. It provides insight into the pathway and intermediates involved in a reaction, allowing chemists to relate the rate constants of individual steps to the overall rate constant of the reaction.