/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 98 If a reaction is zero order in a... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

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.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Using data in Appendix \(4,\) calculate \(\Delta H^{\circ}\) for the reaction $$\mathrm{O}_{3}(g)+\mathrm{NO}(g) \rightarrow \mathrm{O}_{2}(g)+\mathrm{NO}_{2}(g)$$

Write the rate laws for the following elementary steps and identify them as uni-, bi-, or termolecular steps: a. \(\mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightarrow \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g)\) b. \(\mathrm{NO}_{2}(g)+\mathrm{CO}(g) \rightarrow \mathrm{NO}(g)+\mathrm{CO}_{2}(g)\) c. \(2 \mathrm{NO}_{2}(g) \rightarrow \mathrm{NO}_{3}(g)+\mathrm{NO}(g)\)

Nitrite ion reacts with ozone in aqueous solution, producing nitrate ion and oxygen: $$\mathrm{NO}_{2}^{-}(a q)+\mathrm{O}_{3}(g) \rightarrow \mathrm{NO}_{3}^{-}(a q)+\mathrm{O}_{2}(g)$$ The following data were collected for this reaction at \(298 \mathrm{K} .\) Calculate the average reaction rate between 0 and \(100 \mu \mathrm{s}(\text { microseconds })\) and between 200 and \(300 \mu \mathrm{s}\) $$\begin{array}{cc}\text { Time }(\mu \mathrm{s}) & {\left[\mathrm{O}_{3}\right](\mathrm{M})} \\\0 & 1.13 \times 10^{-2} \\\\\hline 100 & 9.93 \times 10^{-3} \\\\\hline 200 & 8.70 \times 10^{-3} \\\\\hline 300 & 8.15 \times 10^{-3} \\\\\hline\end{array}$$

On the basis of the frequency factors and activation energy values of the following two reactions, determine which one will have the larger rate constant at room temperature \((298 \mathrm{K})\). \(\mathrm{O}_{3}(g)+\mathrm{O}(g) \rightarrow \mathrm{O}_{2}(g)+\mathrm{O}_{2}(g)\) \(A=8.0 \times 10^{-12} \mathrm{cm}^{3} /(\text { molecules } \cdot \mathrm{s}) \quad E_{\mathrm{a}}=17.1 \mathrm{kJ} / \mathrm{mol}\) \(\mathrm{O}_{3}(g)+\mathrm{Cl}(g) \rightarrow \mathrm{ClO}(g)+\mathrm{O}_{2}(g)\) \(A=2.9 \times 10^{-11} \mathrm{cm}^{3} /(\text { molecules } \cdot \mathrm{s}) \quad E_{\mathrm{a}}=2.16 \mathrm{kJ} / \mathrm{mol}\)

During the decomposition of dinitrogen pentoxide, $$2 \mathrm{N}_{2} \mathrm{O}_{5}(g) \rightarrow 4 \mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g)$$ how is the rate of consumption of \(\mathrm{N}_{2} \mathrm{O}_{5}\) related to the rate of formation of \(\mathrm{NO}_{2}\) and \(\mathrm{O}_{2} ?\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemistry Branches

Read Explanation

Kinetics

Read Explanation

The Earths Atmosphere

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.