A mechanism for the gas prase step 1 slow: F₂ + CIO2 → FCIO2 + F step 2 fast: F + CIO₂ →→ FCIO2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. F₂ + 2C102 2FC10₂ + er) Greek(lower) Arrows Other Aa (s) (1) (g) (aq) that is Rate = on intermediate? Enter formula. If none, leave box blank: F Þ (3) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A] [B]"..., where '1' is understood (so don't write it) for m, n etc.)
A mechanism for the gas prase step 1 slow: F₂ + CIO2 → FCIO2 + F step 2 fast: F + CIO₂ →→ FCIO2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. F₂ + 2C102 2FC10₂ + er) Greek(lower) Arrows Other Aa (s) (1) (g) (aq) that is Rate = on intermediate? Enter formula. If none, leave box blank: F Þ (3) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A] [B]"..., where '1' is understood (so don't write it) for m, n etc.)
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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![### Reaction Mechanism for Fluorine and Chlorine Dioxide
A mechanism for the gas-phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is:
- **Step 1 (slow):**
\[
\text{F}_2 + \text{ClO}_2 \rightarrow \text{FClO}_2 + \text{F}
\]
- **Step 2 (fast):**
\[
\text{F} + \text{ClO}_2 \rightarrow \text{FClO}_2
\]
**Questions and Instructions:**
1. **What is the equation for the overall reaction?**
Use the smallest integer coefficients possible. If a box is not needed, leave it blank.
\[
\boxed{\text{F}_2} + \boxed{2\text{ClO}_2} \rightarrow \boxed{2\text{FClO}_2} + \boxed{}
\]
2. **What species is an intermediate?**
Enter the formula. If none, leave the box blank:
\[
\boxed{\text{F}}
\]
3. **Complete the rate law for the overall reaction that is consistent with this mechanism.**
*(Use the form k[A]^m[B]^n ..., where "1" is understood (so don’t write it) for m, n, etc.)*
\[
\text{Rate} = \boxed{}
\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9413ee1b-018f-4e4f-9457-fb88f0adac84%2F5f6104ab-e5f8-4a45-871b-986de748ea39%2Fks77bv_processed.png&w=3840&q=75)
Transcribed Image Text:### Reaction Mechanism for Fluorine and Chlorine Dioxide
A mechanism for the gas-phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is:
- **Step 1 (slow):**
\[
\text{F}_2 + \text{ClO}_2 \rightarrow \text{FClO}_2 + \text{F}
\]
- **Step 2 (fast):**
\[
\text{F} + \text{ClO}_2 \rightarrow \text{FClO}_2
\]
**Questions and Instructions:**
1. **What is the equation for the overall reaction?**
Use the smallest integer coefficients possible. If a box is not needed, leave it blank.
\[
\boxed{\text{F}_2} + \boxed{2\text{ClO}_2} \rightarrow \boxed{2\text{FClO}_2} + \boxed{}
\]
2. **What species is an intermediate?**
Enter the formula. If none, leave the box blank:
\[
\boxed{\text{F}}
\]
3. **Complete the rate law for the overall reaction that is consistent with this mechanism.**
*(Use the form k[A]^m[B]^n ..., where "1" is understood (so don’t write it) for m, n, etc.)*
\[
\text{Rate} = \boxed{}
\]
Expert Solution
Step 1
The given two steps of the reaction are:
For a multi-step reaction, the slow step is the rate-determining step.
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