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Chapter 13: Problem 98

If a reaction is zero order in a reactant, does that mean the reactant is never involved in collisions with other reactants? Explain your answer.

Short Answer

Expert verified
Short Answer: No, a zero-order reaction does not indicate that the reactant is not involved in collisions with other reactants. Instead, it indicates that the rate of the reaction is not dependent on the concentration of that specific reactant, possibly due to factors such as the presence of a catalyst or a rate-limiting step that is independent of the concentration of that reactant.

Step by step solution

01

Understanding reaction order

Reaction order is an important aspect of chemical kinetics, which describes the relationship between the concentrations of reactants and the rate of a reaction. It tells us how the rate of a reaction changes with a change in the concentration of one of the reactants. The order of a reaction can be positive, negative, or zero, depending on the nature of the reaction.
02

Definition of zero-order reaction

A zero-order reaction is a type of reaction where the rate of the reaction does not depend on the concentration of any of its reactants. Mathematically, it can be expressed as: rate = k, where k is the rate constant. Since the reaction rate is independent of the concentration of the reactants, the reaction proceeds at a constant rate until one or more reactants are depleted.
03

Collision theory and chemical reactions

According to the collision theory, chemical reactions occur when the reactant molecules collide with one another with sufficient kinetic energy and proper orientation. Not all collisions result in a reaction, but the more frequently molecules collide, the more likely they are to react.
04

Zero-order reaction and collision involvement

The fact that a reaction is zero-order does not mean that the reactant is not involved in collisions with other reactants. Instead, it indicates that the rate of the reaction is not dependent on the concentration of that specific reactant. This could be because the reaction is controlled by another factor, such as the presence of a catalyst or a rate-limiting step that is independent of the concentration of that reactant. In conclusion, a zero-order reaction does not imply that the reactant is never involved in collisions with other reactants. It simply means that the rate of the reaction is not influenced by the concentration of the reactant in question.

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Most popular questions from this chapter

The reaction between \(\mathrm{N}_{2} \mathrm{O}_{5}\) and water is a source of nitric acid in the atmosphere: $$\mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow 2 \mathrm{HNO}_{3}(g)$$ a. The reaction is first order in each reactant. Write the rate law for the reaction. b. When \(\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]=0.132 \mathrm{m} \mathrm{M}\) and \(\left[\mathrm{H}_{2} \mathrm{O}\right]=230 \mathrm{m} M,\) the rate of the reaction is \(4.55 \times 10^{-4} \mathrm{mM} / \mathrm{min} .\) What is the rate constant for the reaction?

Nitrogen and oxygen can combine to form different nitrogen oxides that play a minor role in the chemistry of smog. Write balanced chemical equations for the reactions of \(\mathrm{N}_{2}\) and \(\mathrm{O}_{2}\) that produce (a) \(\mathrm{N}_{2} \mathrm{O}\) and (b) \(\mathrm{N}_{2} \mathrm{O}_{5}\).

Can the concentration of a homogeneous catalyst appear in the rate law for the reaction it catalyzes?

Can the average rate and instantaneous rate of a chemical reaction ever be the same?

Under what circumstances is the activation energy of a reaction proceeding in the forward direction greater than the activation energy of it happening in reverse?
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