Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 16: Problem 31

Why is it necessary, in defining the rate of a reaction, to require that \(\Delta t\) be small?

Short Answer

Expert verified
A small \(\Delta t\) is necessary in defining the rate of a reaction as it measures the instantaneous reaction rate at a specific point in time. If \(\Delta t\) is large, the calculated rate might not represent the rate at a particular instant due to varying concentrations of the reactants or products during that interval.

Step by step solution

01

Understand the basic concept of reaction rate

The rate of a reaction at a moment is the speed at which a reaction is proceeding. It is usually defined by the change in concentration of reactants or products over a certain period of time. The rate of reaction is often given as \(-\frac{\Delta [A]}{\Delta t}\) for a reactant A, where \([A]\) is the concentration of A and \(\Delta t\) is a small interval of time.
02

Define the term 'small \(\Delta t\)'

The term 'small \(\Delta t\)' refers to an infinitesimally small time interval. In the context of reaction rates, small \(\Delta t\) is used to calculate instantaneous reaction rates, which refers to the rate of reaction at a specific instant or point in time.
03

Elaborate the need for small \(\Delta t\)

In reactions, concentrations of reactants change all the time. So, if we take too large a \(\Delta t\), the average rate over that interval could differ significantly from the rate at any particular instant within that interval. Using a small \(\Delta t\) ensures that changes in concentrations are small enough, providing a more representative, instantaneous rate of reaction.

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

Boilers are sometimes used to heat large buildings. Deposits of \(\mathrm{CaCO}_{3}, \mathrm{MgCO}_{3},\) and \(\mathrm{FeCO}_{3}\) can hinder the boiler operation. Aqueous solutions of hydrochloric acid are commonly used to remove these deposits. The general equation for the reaction is written below. $$\begin{array}{c}{\mathrm{MCO}_{3}(s)+2 \mathrm{H}_{3} \mathrm{O}^{+}(a q) \rightarrow} \\ {\mathrm{M}^{2+}(a q)+3 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g)}\end{array}$$ In the equation, M stands for Ca, Mg, or Fe. Design an experiment to determine the effect of various HCl concentrations on the rates of this reaction. Present your design to the class.

What is the reaction order if the reaction rate triples when the concentration of a reactant is increased by a factor of 3\(?\)

How do enzymes differ from other catalysts?

Write the general expression for the rate law of a reaction with three reactants \(\mathrm{A}, \mathrm{B},\) and \(\mathrm{C}\) .

Would you expect the concentration of a catalyst to appear in the rate law of a catalyzed reaction? Explain.
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

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.

Sign-up for free