**Order and Rate Law of a Reaction**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:\[ \text{rate} = k[\text{NO}_2]^2 \]The exponent "2" is used because the reaction involves two NO₂ molecules. The rate law for step 2 is:\[ \text{rate} = k[\text{NO}_3]^1[\text{CO}]^1 = k[\text{NO}_3][\text{CO}] \]Because the reaction involves only one molecule of each reactant, the exponents are omitted.---**Analyzing a New Reaction**Consider the following elementary steps that make up the mechanism of a certain reaction:1. 2A → B + C2. B + D → E + C---**Part A****What is the overall reaction?**Express your answer as a chemical equation.[A chemical reaction does not occur for this question.]

In this reaction B is intermediate. Intermediate is species which formed during reaction but is not…

Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1. 2A-B+C 2. B+ D→E+ C Part A What is the overall reaction? Express your answer as a chemical equation.

Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1. 2A-B+C 2. B+ D→E+ C Part A What is the overall reaction? Express your answer as a chemical equation.

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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Question

**Order and Rate Law of a Reaction**

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:

\[ \text{rate} = k[\text{NO}_2]^2 \]

The exponent "2" is used because the reaction involves two NO₂ molecules. The rate law for step 2 is:

\[ \text{rate} = k[\text{NO}_3]^1[\text{CO}]^1 = k[\text{NO}_3][\text{CO}] \]

Because the reaction involves only one molecule of each reactant, the exponents are omitted.

---

**Analyzing a New Reaction**

Consider the following elementary steps that make up the mechanism of a certain reaction:

1. 2A → B + C
2. B + D → E + C

---

**Part A**

**What is the overall reaction?**

Express your answer as a chemical equation.

[A chemical reaction does not occur for this question.]

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