The following is a proposed mechanism for the gas phase decomposition of nitryl chloride. step 1 fast: NO₂CINO₂ + CI step 2 slow: NO₂CI+ CI →→→→ NO₂ + Cl₂ (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + → + (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A][B]n..., where '1' is understood (so don't write it if it's a '1') for m, n etc. Rate =
The following is a proposed mechanism for the gas phase decomposition of nitryl chloride. step 1 fast: NO₂CINO₂ + CI step 2 slow: NO₂CI+ CI →→→→ NO₂ + Cl₂ (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + → + (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A][B]n..., where '1' is understood (so don't write it if it's a '1') for m, n etc. Rate =
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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![The following is a proposed mechanism for the gas phase decomposition of nitryl chloride.
**Step 1**
*fast:*
\( \text{NO}_2\text{Cl} \rightleftharpoons \text{NO}_2 + \text{Cl} \)
**Step 2**
*slow:*
\( \text{NO}_2\text{Cl} + \text{Cl} \rightarrow \text{NO}_2 + \text{Cl}_2 \)
---
**(1)** What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank.
\[
\boxed{} \quad + \quad \boxed{} \quad \longrightarrow \quad \boxed{} \quad + \quad \boxed{}
\]
**(2)** Enter the formula of any species that acts as a reaction intermediate. If none, leave the box blank:
\[
\boxed{}
\]
**(3)** Complete the rate law for the overall reaction that is consistent with this mechanism.
Use the form \( k[A]^m[B]^n \ldots \), where '1' is understood (*so don't write it if it's a '1'*) for \( m, n \), etc.
**Rate** = \(\boxed{} \)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7a354f1c-cdfd-41e5-a863-9a86a504af1c%2Fa4ae7812-482f-453c-94ad-2aa3a950a114%2Fpt345d_processed.png&w=3840&q=75)
Transcribed Image Text:The following is a proposed mechanism for the gas phase decomposition of nitryl chloride.
**Step 1**
*fast:*
\( \text{NO}_2\text{Cl} \rightleftharpoons \text{NO}_2 + \text{Cl} \)
**Step 2**
*slow:*
\( \text{NO}_2\text{Cl} + \text{Cl} \rightarrow \text{NO}_2 + \text{Cl}_2 \)
---
**(1)** What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank.
\[
\boxed{} \quad + \quad \boxed{} \quad \longrightarrow \quad \boxed{} \quad + \quad \boxed{}
\]
**(2)** Enter the formula of any species that acts as a reaction intermediate. If none, leave the box blank:
\[
\boxed{}
\]
**(3)** Complete the rate law for the overall reaction that is consistent with this mechanism.
Use the form \( k[A]^m[B]^n \ldots \), where '1' is understood (*so don't write it if it's a '1'*) for \( m, n \), etc.
**Rate** = \(\boxed{} \)
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