/*! 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 3 What are the advantages of measu... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 14: Problem 3

What are the advantages of measuring the initial rate of a reaction?

Short Answer

Expert verified
The advantages of measuring the initial rate of a reaction include: 1) accurate determination of the reaction rate, 2) gaining insight into the reaction mechanism, and 3) enabling manipulation of reaction conditions for optimal results.

Step by step solution

01

Understanding the Concept

The initial rate of a reaction refers to the change in concentration of a reactant or a product per unit time at the start of the reaction - essentially, the speed at which a reaction proceeds when it just begins. This rate can be measured before the reaction reaches equilibrium.
02

Advantage 1: Accurate Determination of Reaction Rate

One advantage of measuring the initial rate of a reaction is that it leads to an accurate determination of the reaction rate. Since measurements are taken before the reaction starts to slow down due to depletion of reactants, it eliminates the influence of back reactions or side reactions.
03

Advantage 2: Insight into Reaction Mechanism

Measuring the initial rate of reaction helps to understand the reaction mechanism. It allows one to infer how reactants are transformed into products step-by-step by understanding the order of reaction, which can provide insight into the sequence of steps that make up the overall reaction.
04

Advantage 3: Enabling Manipulation of Reaction Conditions

Understanding the initial rate can enable scientists to manipulate the reaction conditions such as concentration of reactants, temperature etc., for desired speed and results. It aids in designing efficient industrial processes by optimizing reaction conditions for maximum yield at minimal cost.

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

The rate law for the reaction $$ \mathrm{NH}_{4}^{+}(a q)+\mathrm{NO}_{2}^{-}(a q) \longrightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) $$ is given by rate \(=k\left[\mathrm{NH}_{4}^{+}\right]\left[\mathrm{NO}_{2}^{-}\right]\). At \(25^{\circ} \mathrm{C},\) the rate constant is \(3.0 \times 10^{-4} / M \cdot\) s. Calculate the rate of the reaction at this temperature if \(\left[\mathrm{NH}_{4}^{+}\right]=0.26 \mathrm{M}\) and \(\left[\mathrm{NO}_{2}^{-}\right]=0.080 \mathrm{M}\)

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

The thermal decomposition of phosphine \(\left(\mathrm{PH}_{3}\right)\) into phosphorus and molecular hydrogen is a first-order reaction: $$ 4 \mathrm{PH}_{3}(g) \longrightarrow \mathrm{P}_{4}(g)+6 \mathrm{H}_{2}(g) $$ The half-life of the reaction is 35.0 s at \(680^{\circ} \mathrm{C}\). Calculate (a) the first-order rates constant for the reaction and (b) the time required for 95 percent of the phosphine to decompose.

The reaction \(\mathrm{H}+\mathrm{H}_{2} \longrightarrow \mathrm{H}_{2}+\mathrm{H}\) has been studied for many years. Sketch a potential-energy-versusreaction-progress diagram for this reaction.

Consider the reaction $$ \mathrm{A} \longrightarrow \mathrm{B} $$ The rate of the reaction is \(1.6 \times 10^{-2} M / \mathrm{s}\) when the concentration of A is \(0.35 M\). Calculate the rate constant if the reaction is (a) first order in \(\mathrm{A},\) (b) second order in A.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Kinetics

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.