toshiki-notebook/assets/academic_chemistry_notes_12-5.md.6f7d3f5c.lean.js

import{_ as l}from"./chunks/PageInfo.vue_vue_type_script_setup_true_lang.250b3e56.js";import{_ as e,o as n,c as m,H as i,k as s,a}from"./chunks/framework.b7580407.js";import"./chunks/commonjsHelpers.725317a4.js";const cs=JSON.parse('{"title":"12-5: Reaction Mechanism","description":"","frontmatter":{"title":"12-5: Reaction Mechanism","editLink":true,"lastUpdated":true,"showArticleMetadata":true,"categories":["Chemistry"],"keywords":["chemistry","reaction","mechanism","reaction-mechanism","tutorial","explanation","textbook","reference"]},"headers":[],"relativePath":"academic/chemistry/notes/12-5.md","filePath":"academic/chemistry/notes/12-5.md","lastUpdated":1711521027000}'),r={name:"academic/chemistry/notes/12-5.md"},c=s("h1",{id:"_12-5-reaction-mechanism",tabindex:"-1"},[a("12-5: Reaction Mechanism "),s("a",{class:"header-anchor",href:"#_12-5-reaction-mechanism","aria-label":'Permalink to "12-5: Reaction Mechanism"'},"​")],-1),p=s("h2",{id:"_12-5-1-learning-objectives",tabindex:"-1"},[a("12-5-1: Learning Objectives "),s("a",{class:"header-anchor",href:"#_12-5-1-learning-objectives","aria-label":'Permalink to "12-5-1: Learning Objectives"'},"​")],-1),h=s("div",{class:"tip custom-block"},[s("p",{class:"custom-block-title"},"Learning Objectives"),s("p",null,"One of the major reasons for studying chemical kinetics is to use measurements of the macroscopic properties of a system, such as the rate of change in the concentration of reactants or products with time, to discover the sequence of events that occur at the molecular level during a reaction. This molecular description is the mechanism of the reaction; it describes how individual atoms, ions, or molecules interact to form particular products. The stepwise changes are collectively called the reaction mechanism.")],-1),o=s("p",null,"In an internal combustion engine, for example, isooctane reacts with oxygen to give carbon dioxide and 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It is more likely that a complex series of reactions takes place in a stepwise fashion. Each individual reaction, which is called an elementary reaction, involves one, two, or (rarely) three atoms, molecules, or ions. The overall sequence of elementary reactions is the mechanism of the reaction. The sum of the individual steps, or elementary reactions, in the mechanism must give the balanced chemical equation for the overall reaction.",-1),d=s("p",null,"The overall sequence of elementary reactions is the mechanism of the reaction.",-1),v=s("h2",{id:"_12-5-2-molecularity-and-the-rate-determining-step",tabindex:"-1"},[a("12-5-2: Molecularity and the Rate-Determining Step "),s("a",{class:"header-anchor",href:"#_12-5-2-molecularity-and-the-rate-determining-step","aria-label":'Permalink to "12-5-2: Molecularity and the Rate-Determining Step"'},"​")],-1),y=s("p",null,"To demonstrate how the analysis of elementary reactions helps us determine the overall reaction mechanism, we will examine the much simpler reaction of carbon monoxide with nitrogen 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It is formed as a product of the first step but is consumed in the second step.")],-1),N=s("p",null,"The sum of the elementary reactions in a reaction mechanism must give the overall balanced chemical equation of the reaction.",-1),C=s("h2",{id:"_12-5-3-using-molecularity-to-describe-a-rate-law",tabindex:"-1"},[a("12-5-3: Using Molecularity to Describe a Rate Law "),s("a",{class:"header-anchor",href:"#_12-5-3-using-molecularity-to-describe-a-rate-law","aria-label":'Permalink to "12-5-3: Using Molecularity to Describe a Rate Law"'},"​")],-1),L=s("p",null,"The molecularity of an elementary reaction is the number of molecules that collide during that step in the mechanism. If there is only a single reactant molecule in an elementary reaction, that step is designated as unimolecular; if there are two reactant molecules, it is bimolecular; and if there are three reactant molecules (a relatively rare situation), it is termolecular. Elementary reactions that involve the simultaneous collision of more than three molecules are highly improbable and have never been observed experimentally. (To understand why, try to make three or more marbles or pool balls collide with one another simultaneously!)",-1),A=s("div",{class:"warning custom-block"},[s("p",{class:"custom-block-title"},"About the image"),s("p",null,"The Basis for Writing Rate Laws of Elementary Reactions. This diagram illustrates how the number of possible collisions per unit time between two reactant species, A and B, depends on the number of A and B particles present. The number of collisions between A and B particles increases as the product of the number of particles, not as the sum. This is why the rate law for an elementary reaction depends on the product of the concentrations of the species that collide in that step. 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