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Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1. 3X→E+F 2. E+ M→F+N Part A What is the overall reaction?

Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1. 3X→E+F 2. E+ M→F+N Part A What is the overall reaction?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Review I Constants I Periodic Table Learning Goal: To understand how elementary steps make up a mechanism and how the rate law for an elementary step Order and rate law of a reaction can be determined. The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is Very often, a reaction does not tell us the whole story. For instance, the reaction NO2(9) + CO(9)→NO(g)+ CO2(g) rate = k[NO2]2 does not involve a collision between an NO, molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: The exponent "2" is used because the reaction involves two NO2 molecules. The rate law for step 2 is rate = k[NO3]'[CO]* = k[NO3][CO] 1. NO2(9) + NO2(9)→NO3(9)+NO(g) 2. NO3(g) + CO(9)→CO2(9) +NO2(g9) because the reaction involves only one molecule of each reactant the exponents are omitted. Each individual step is called an elementary step. Together, these elementary steps are called the reaction mechanism. Analyzing a new reaction Overall, the resulting reaction is Consider the following elementary steps that make up the mechanism of a certain reaction: NO2 (9) + CO(g)→NO(g)+ CO2(g) 1. 3X→E+F 2. E + M→F +N Notice that in the elementary steps NO3 appears both as a product and then as a reactant; therefore it cancels out mical equation. NO3 is called a reaction intermediate. Also notice that 2 molecules of Part A NO2 appear in the reactants of the first step and 1 molecule of NO2 appears as product of the second step, the net effect leaves only 1 molecule of NO2 as What is the overall reaction?
Transcribed Image Text:Review I Constants I Periodic Table Learning Goal: To understand how elementary steps make up a mechanism and how the rate law for an elementary step Order and rate law of a reaction can be determined. The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is Very often, a reaction does not tell us the whole story. For instance, the reaction NO2(9) + CO(9)→NO(g)+ CO2(g) rate = k[NO2]2 does not involve a collision between an NO, molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: The exponent "2" is used because the reaction involves two NO2 molecules. The rate law for step 2 is rate = k[NO3]'[CO]* = k[NO3][CO] 1. NO2(9) + NO2(9)→NO3(9)+NO(g) 2. NO3(g) + CO(9)→CO2(9) +NO2(g9) because the reaction involves only one molecule of each reactant the exponents are omitted. Each individual step is called an elementary step. Together, these elementary steps are called the reaction mechanism. Analyzing a new reaction Overall, the resulting reaction is Consider the following elementary steps that make up the mechanism of a certain reaction: NO2 (9) + CO(g)→NO(g)+ CO2(g) 1. 3X→E+F 2. E + M→F +N Notice that in the elementary steps NO3 appears both as a product and then as a reactant; therefore it cancels out mical equation. NO3 is called a reaction intermediate. Also notice that 2 molecules of Part A NO2 appear in the reactants of the first step and 1 molecule of NO2 appears as product of the second step, the net effect leaves only 1 molecule of NO2 as What is the overall reaction?
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