**Decomposition of Nitrosyl Chloride at 400 K** The gas phase decomposition reaction for nitrosyl chloride (NOCl) at 400 K is as follows: \[ \text{2 NOCl(g)} \rightarrow \text{2 NO(g)} + \text{1/2 Cl}_{2}\text{(g)} \] This reaction is second order in NOCl, with a rate constant of \( \text{5.90} \times \text{10}^{-4} \, \text{M}^{-1}\text{s}^{-1} \). Given: - The initial concentration of NOCl is \( \text{6.78} \times \text{10}^{-2} \, \text{M} \). Problem: Calculate the concentration of NOCl after \( \text{1.66} \times \text{10}^{5} \) seconds have passed. [Submit Answer] [Retry Entire Group] More group attempts remaining *Note: The section above does not include any graphs or diagrams but provides the details necessary for solving a reaction rate problem, specifically that of a second-order reaction.* **The Decomposition of Ammonia on a Platinum Surface at 856°C** The chemical reaction is represented as follows: \[ \text{NH}_3 \rightarrow \frac{1}{2} \text{N}_2 + \frac{3}{2} \text{H}_2 \] The reaction is zero order in \(\text{NH}_3\) with a rate constant of \(1.50 \times 10^{-6}\) M/s. If the initial concentration of \(\text{NH}_3\) is \(1.18 \times 10^{-2}\) M, determine how many seconds will pass until the concentration of \(\text{NH}_3\) reduces to \(3.45 \times 10^{-3}\) M. **Options:** - Submit Answer - Retry Entire Group (9 more group attempts remaining) **Navigation:** - Previous - Next **Support:** - [Email instructor] - [Save and Exit] **Note:** There are no graphs or diagrams to explain for this image.
**Decomposition of Nitrosyl Chloride at 400 K** The gas phase decomposition reaction for nitrosyl chloride (NOCl) at 400 K is as follows: \[ \text{2 NOCl(g)} \rightarrow \text{2 NO(g)} + \text{1/2 Cl}_{2}\text{(g)} \] This reaction is second order in NOCl, with a rate constant of \( \text{5.90} \times \text{10}^{-4} \, \text{M}^{-1}\text{s}^{-1} \). Given: - The initial concentration of NOCl is \( \text{6.78} \times \text{10}^{-2} \, \text{M} \). Problem: Calculate the concentration of NOCl after \( \text{1.66} \times \text{10}^{5} \) seconds have passed. [Submit Answer] [Retry Entire Group] More group attempts remaining *Note: The section above does not include any graphs or diagrams but provides the details necessary for solving a reaction rate problem, specifically that of a second-order reaction.* **The Decomposition of Ammonia on a Platinum Surface at 856°C** The chemical reaction is represented as follows: \[ \text{NH}_3 \rightarrow \frac{1}{2} \text{N}_2 + \frac{3}{2} \text{H}_2 \] The reaction is zero order in \(\text{NH}_3\) with a rate constant of \(1.50 \times 10^{-6}\) M/s. If the initial concentration of \(\text{NH}_3\) is \(1.18 \times 10^{-2}\) M, determine how many seconds will pass until the concentration of \(\text{NH}_3\) reduces to \(3.45 \times 10^{-3}\) M. **Options:** - Submit Answer - Retry Entire Group (9 more group attempts remaining) **Navigation:** - Previous - Next **Support:** - [Email instructor] - [Save and Exit] **Note:** There are no graphs or diagrams to explain for this image.
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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![**Decomposition of Nitrosyl Chloride at 400 K**
The gas phase decomposition reaction for nitrosyl chloride (NOCl) at 400 K is as follows:
\[ \text{2 NOCl(g)} \rightarrow \text{2 NO(g)} + \text{1/2 Cl}_{2}\text{(g)} \]
This reaction is second order in NOCl, with a rate constant of \( \text{5.90} \times \text{10}^{-4} \, \text{M}^{-1}\text{s}^{-1} \).
Given:
- The initial concentration of NOCl is \( \text{6.78} \times \text{10}^{-2} \, \text{M} \).
Problem:
Calculate the concentration of NOCl after \( \text{1.66} \times \text{10}^{5} \) seconds have passed.
[Submit Answer]
[Retry Entire Group]
More group attempts remaining
*Note: The section above does not include any graphs or diagrams but provides the details necessary for solving a reaction rate problem, specifically that of a second-order reaction.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F120dfaba-c029-420e-add2-1a0674ef38e5%2F2a686597-9afd-4206-b908-c1bebd980a92%2Fsrmsvut.jpeg&w=3840&q=75)
Transcribed Image Text:**Decomposition of Nitrosyl Chloride at 400 K**
The gas phase decomposition reaction for nitrosyl chloride (NOCl) at 400 K is as follows:
\[ \text{2 NOCl(g)} \rightarrow \text{2 NO(g)} + \text{1/2 Cl}_{2}\text{(g)} \]
This reaction is second order in NOCl, with a rate constant of \( \text{5.90} \times \text{10}^{-4} \, \text{M}^{-1}\text{s}^{-1} \).
Given:
- The initial concentration of NOCl is \( \text{6.78} \times \text{10}^{-2} \, \text{M} \).
Problem:
Calculate the concentration of NOCl after \( \text{1.66} \times \text{10}^{5} \) seconds have passed.
[Submit Answer]
[Retry Entire Group]
More group attempts remaining
*Note: The section above does not include any graphs or diagrams but provides the details necessary for solving a reaction rate problem, specifically that of a second-order reaction.*
![**The Decomposition of Ammonia on a Platinum Surface at 856°C**
The chemical reaction is represented as follows:
\[ \text{NH}_3 \rightarrow \frac{1}{2} \text{N}_2 + \frac{3}{2} \text{H}_2 \]
The reaction is zero order in \(\text{NH}_3\) with a rate constant of \(1.50 \times 10^{-6}\) M/s.
If the initial concentration of \(\text{NH}_3\) is \(1.18 \times 10^{-2}\) M, determine how many seconds will pass until the concentration of \(\text{NH}_3\) reduces to \(3.45 \times 10^{-3}\) M.
**Options:**
- Submit Answer
- Retry Entire Group (9 more group attempts remaining)
**Navigation:**
- Previous
- Next
**Support:**
- [Email instructor]
- [Save and Exit]
**Note:** There are no graphs or diagrams to explain for this image.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F120dfaba-c029-420e-add2-1a0674ef38e5%2F2a686597-9afd-4206-b908-c1bebd980a92%2Fw0ogihk.jpeg&w=3840&q=75)
Transcribed Image Text:**The Decomposition of Ammonia on a Platinum Surface at 856°C**
The chemical reaction is represented as follows:
\[ \text{NH}_3 \rightarrow \frac{1}{2} \text{N}_2 + \frac{3}{2} \text{H}_2 \]
The reaction is zero order in \(\text{NH}_3\) with a rate constant of \(1.50 \times 10^{-6}\) M/s.
If the initial concentration of \(\text{NH}_3\) is \(1.18 \times 10^{-2}\) M, determine how many seconds will pass until the concentration of \(\text{NH}_3\) reduces to \(3.45 \times 10^{-3}\) M.
**Options:**
- Submit Answer
- Retry Entire Group (9 more group attempts remaining)
**Navigation:**
- Previous
- Next
**Support:**
- [Email instructor]
- [Save and Exit]
**Note:** There are no graphs or diagrams to explain for this image.
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