/*! 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 19 The central idea of the collisio... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 12: Problem 19

The central idea of the collision model is that molecules must collide in order to react. Give two reasons why not all collisions of reactant molecules result in product formation.

Short Answer

Expert verified
Not all collisions of reactant molecules result in product formation due to two main reasons: firstly, the collisions might not have sufficient activation energy, which is the minimum energy required for a successful reaction; secondly, the reactant molecules might collide at an incorrect orientation, preventing efficient overlapping of the reacting orbitals and thus, hindering the bonding process.

Step by step solution

01

Understand the Collision Theory

The collision model proposes that for a chemical reaction to occur, the reactant molecules must collide with each other. However, not all collisions will lead to a reaction, and certain conditions must be met for the reaction to proceed.
02

Reason 1: Insufficient Activation Energy

The reactant molecules need to have a minimum amount of energy for a successful reaction, which is called the activation energy. Activation energy is the energy barrier that needs to be overcome for a reaction to occur. When molecules collide with less than the required activation energy, they may simply bounce off each other and not react.
03

Reason 2: Incorrect Orientation

The reactant molecules must also collide at the correct orientation (approach angle) for a successful reaction. The collision orientation determines the efficient overlap between the reacting orbitals of the molecules, allowing the bonding process to take place. If the reactant molecules collide at an incorrect orientation, they may bounce off each other and not form a 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.

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

A certain reaction has the following general form: $$ \mathrm{aA} \longrightarrow \mathrm{bB} $$ At a particular temperature and \([\mathrm{A}]_{0}=2.00 \times 10^{-2} M,\) con- centration versus time data were collected for this reaction, and a plot of \(\ln [\mathrm{A}]\) versus time resulted in a straight line with a slope value of \(-2.97 \times 10^{-2} \mathrm{min}^{-1}\) . a. Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction. b. Calculate the half-life for this reaction. c. How much time is required for the concentration of A to decrease to \(2.50 \times 10^{-3} M ?\)

In the gas phase, the production of phosgene from chlorine and carbon monoxide is assumed to proceed by the following mechanism: $$ \mathrm{Cl}_{2} \stackrel{k_{1}}{\rightleftharpoons_{k_{1}}} 2 \mathrm{Cl} $$ $$ \mathrm{Cl}+\mathrm{CO} \stackrel{k_{2}}{\leftrightharpoons_{k-2}} \mathrm{COCl} $$ $$ \mathrm{COCl}+\mathrm{Cl}_{2} \stackrel{k_{3}}{\longrightarrow} \mathrm{COCl}_{2}+\mathrm{Cl} $$ $$ 2 \mathrm{Cl} \stackrel{k}{\longrightarrow} \mathrm{Cl}_{2} $$ Overall reaction: \(\mathrm{CO}+\mathrm{Cl}_{2} \longrightarrow \mathrm{COCl}_{2}\) a. Write the rate law for this reaction. b. Which species are intermediates?

The combustion of carbohydrates and the combustion of fats are both exothermic processes, yet the combustion of carbohydrates is a faster process. How can this be?

The reaction $$ \mathrm{A} \longrightarrow \mathrm{B}+\mathrm{C} $$ is known to be zero order in A and to have a rate constant of \(5.0 \times 10^{-2} \mathrm{mol} / \mathrm{L} \cdot \mathrm{s}\) at \(25^{\circ} \mathrm{C}\) . An experiment was run at \(25^{\circ} \mathrm{C}\) where \([\mathrm{A}]_{0}=1.0 \times 10^{-3} \mathrm{M} .\) a. Write the integrated rate law for this reaction. b. Calculate the half-life for the reaction. c. Calculate the concentration of \(\mathrm{B}\) after \(5.0 \times 10^{-3} \mathrm{s}\) has elapsed assuming \([\mathrm{B}]_{0}=0\)

The decomposition of iodoethane in the gas phase proceeds according to the following equation: $$ \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{I}(g) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{H}(g) $$ At \(660 . \mathrm{K}, k=7.2 \times 10^{-4} \mathrm{s}^{-1} ;\) at \(720 . \mathrm{K}, k=1.7 \times 10^{-2} \mathrm{s}^{-1}\) What is the value of the rate constant for this first-order decomposition at \(325^{\circ} \mathrm{C} ?\) If the initial pressure of iodoethane is 894 torr at \(245^{\circ} \mathrm{C},\) what is the pressure of iodoethane after three half-lives?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Making Measurements

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.