**Learning Goal:**To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined.### ContextVery often, a reaction does not tell us the whole story. For instance, the reaction:\[ \text{NO}_2(g) + \text{CO}(g) \rightarrow \text{NO}(g) + \text{CO}_2(g) \]does not involve a collision between an NO\(_2\) molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps:1. \[ \text{NO}_2(g) + \text{NO}_2(g) \rightarrow \text{NO}_3(g) + \text{NO}(g) \]2. \[ \text{NO}_3(g) + \text{CO}(g) \rightarrow \text{CO}_2(g) + \text{NO}_2(g) \]Each individual step is called an elementary step. Together, these elementary steps are called the reaction mechanism.### Overall ReactionThe resulting reaction is:\[ \text{NO}_2(g) + \text{CO}(g) \rightarrow \text{NO}(g) + \text{CO}_2(g) \]Notice that in the elementary steps, NO\(_3\) appears both as a product and then as a reactant, therefore it cancels out of the final chemical equation. NO\(_3\) is called a reaction intermediate. Also, notice that 2 molecules of NO\(_2\) appear in the reactants of the first step and 1 molecule of NO\(_2\) appears as product of the second step, the net effect is to use up 1 molecule of NO\(_2\) as a reactant in the net equation.### ExplanationThe rate law is the expression for "how the molecules collide" in a reaction. For example, the rate law for the first elementary reaction is \([A][B]\) because molecules A and B must collide for the reaction to occur. Such a reaction would be bimolecular for the same reason. Unimolecular reactions involve only one molecule in the reactants. Through rare, collisions among three molecules can occur. Such a reaction would be called termolecular.---### Questions**Part C**- What is the rate law for **Week 1 Assignment: Chemical Kinetics****Mechanisms and Molecularity****Learning Goal:** To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined.Very often, a reaction does not tell us the whole story. For instance, the reaction:\[ \text{NO}_2(g) + \text{CO}(g) \rightarrow \text{NO}(g) + \text{CO}_2(g) \]does not involve a collision between an NO\(_2\) molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps:1. \[ \text{NO}_2(g) + \text{NO}_2(g) \rightarrow \text{NO}_3(g) + \text{NO}(g) \]2. \[ \text{NO}_3(g) + \text{CO}(g) \rightarrow \text{NO}_2(g) + \text{CO}_2(g) \]Each individual step is called an *elementary step*. Together, these elementary steps are called the *reaction mechanism*.Overall, the resulting reaction is:\[ \text{NO}_2(g) + \text{CO}(g) \rightarrow \text{NO}(g) + \text{CO}_2(g) \]Notice that in the elementary steps NO\(_2\) appears both as a product and then as a reactant, therefore it cancels out of the final chemical equation. NO\(_3\) is called a *reaction intermediate*. Also notice that 2 molecules of NO\(_2\) appear in the reactants of the first step and 1 molecule of NO\(_2\) appears as product of the second step, the net effect leaves only 1 molecule of NO\(_2\) as a reactant in the net equation.*Molecularity* is the proper term for "how the molecules collide" in a reaction. For example, step 1 is bimolecular because it involves the collision of two molecules. Step 2 is also bimolecular for the same reason. Unimolecular reactions involve one molecule in the reactants. Finally, collisions among three molecules can occur. Such a reaction would be called termolecular.**Order and rate law of a reaction**The overall order of an elementary step directly corresponds

Answered: ep By 4 e uld Analyzing a new reaction…

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...