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Chapter 14: Problem 7

Explain what is meant by the rate law of a reaction.

Short Answer

Expert verified
The rate law of a reaction is a mathematical equation that relates the rate of a chemical reaction to the concentrations of its reactants. It is empirically determined and usually takes the form of 'Rate = k \([A]^m \times [B]^n\)'. The rate law models how a reaction will proceed over time, enabling control over reaction rates and gaining insights about the reaction mechanism and the effect of temperature.

Step by step solution

01

Define the rate law

The rate law of a reaction is a mathematical expression that illustrates the relationship between the rate at which a chemical reaction proceeds and the concentration of the reactants. As such, the rate law is a crucial component in determining the kinetics, or speed, of a chemical reaction.
02

Explain the construction of a rate law

Rate laws are determined experimentally and are usually of the form 'Rate = k \([A]^m \times [B]^n\)', where 'Rate' denotes the rate of the reaction, 'k' denotes the rate constant for the reaction, '[A]' and '[B]' denotes the concentrations of the reactants and 'm' and 'n' denote the orders of the reaction with respect to the reactants A and B respectively. The overall order of reaction is the sum of individual orders (m + n). The orders of reaction represent the effect of reactant concentrations on the rate of reaction and can be 0, 1, 2 or sometimes fractions.
03

Discuss the significance of the rate law

The rate law is significant because it allows scientists to model how a reaction will proceed over time. This has practical importance in a wide array of fields, from designing industrial processes to understanding biological systems. By controlling the concentrations of reactants, the rate of a reaction can be manipulated. Additionally, from the rate constant, the rate law also allows information about the reaction mechanism and the effect of temperature on reaction rate to be obtained.

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Most popular questions from this chapter

(a) What can you deduce about the activation energy of a reaction if its rate constant changes significantly with a small change in temperature? (b) If a bimolecular reaction occurs every time an A and a B molecule collide, what can you say about the orientation factor and activation energy of the reaction?

Consider the zero-order reaction \(\mathrm{A} \longrightarrow\) product. (a) Write the rate law for the reaction. (b) What are the units for the rate constant? (c) Plot the rate of the reaction versus [A].

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Define activation energy. What role does activation energy play in chemical kinetics?

What is meant by the rate of a chemical reaction?
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