The reaction of nitrogen dioxide with carbon monoxide NO, + CONO0 + CO2 is second order in NO, and zero order in CO. Complete the rate law for this reaction in the box below, Use the form k[A]™[B]"... , where 'l' is understood for m, n . (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 0.780 M's. Using this value for the rate constant, the rate of the reaction when [NO,] = 0.460 M and [CO] = 0.372 M would be Ms!.
The reaction of nitrogen dioxide with carbon monoxide NO, + CONO0 + CO2 is second order in NO, and zero order in CO. Complete the rate law for this reaction in the box below, Use the form k[A]™[B]"... , where 'l' is understood for m, n . (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 0.780 M's. Using this value for the rate constant, the rate of the reaction when [NO,] = 0.460 M and [CO] = 0.372 M would be Ms!.
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 Reaction of Nitrogen Dioxide with Carbon Monoxide**
**Reaction:**
\[ \text{NO}_2 + \text{CO} \rightarrow \text{NO} + \text{CO}_2 \]
- The reaction is second order in \(\text{NO}_2\) and zero order in \(\text{CO}\).
**Rate Law:**
Complete the rate law for this reaction in the box below. Use the form \( k[\text{A}]^m[\text{B}]^n \ldots \), where '1' is understood for \( m, n \ldots \) (do not enter 1) and concentrations taken to the zero power do not appear.
**Rate =**
\[ k[\text{NO}_2]^2 \]
**Experimental Determination:**
In an experiment to determine the rate law, the rate constant was determined to be \( 0.780 \, \text{M}^{-1}\text{s}^{-1} \).
Using this value for the rate constant, the rate of the reaction when \([\text{NO}_2] = 0.400 \, \text{M}\) and \([\text{CO}] = 0.372 \, \text{M}\) would be:
**Rate =**
\(k[\text{NO}_2]^2 = 0.780 \times (0.400)^2 = 0.1248 \, \text{Ms}^{-1}\).
(Note: Since CO is zero order, its concentration does not affect the rate and does not appear in the rate law.)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc0168238-e244-4a34-84ac-e572ee66fc4c%2Fb5450d95-4b0c-487f-a40a-bfbf72484767%2Fc7uj7qt_processed.png&w=3840&q=75)
Transcribed Image Text:**The Reaction of Nitrogen Dioxide with Carbon Monoxide**
**Reaction:**
\[ \text{NO}_2 + \text{CO} \rightarrow \text{NO} + \text{CO}_2 \]
- The reaction is second order in \(\text{NO}_2\) and zero order in \(\text{CO}\).
**Rate Law:**
Complete the rate law for this reaction in the box below. Use the form \( k[\text{A}]^m[\text{B}]^n \ldots \), where '1' is understood for \( m, n \ldots \) (do not enter 1) and concentrations taken to the zero power do not appear.
**Rate =**
\[ k[\text{NO}_2]^2 \]
**Experimental Determination:**
In an experiment to determine the rate law, the rate constant was determined to be \( 0.780 \, \text{M}^{-1}\text{s}^{-1} \).
Using this value for the rate constant, the rate of the reaction when \([\text{NO}_2] = 0.400 \, \text{M}\) and \([\text{CO}] = 0.372 \, \text{M}\) would be:
**Rate =**
\(k[\text{NO}_2]^2 = 0.780 \times (0.400)^2 = 0.1248 \, \text{Ms}^{-1}\).
(Note: Since CO is zero order, its concentration does not affect the rate and does not appear in the rate law.)
![**The reaction for the formation of phosgene from carbon monoxide and chlorine**
\[ \text{CO} + \text{Cl}_2 \longrightarrow \text{COCl}_2 \]
is first order in CO and second order overall.
**Complete the rate law for this reaction in the box below.**
Use the form k[A]^m[B]^n..., where '1' is understood for m, n... *(don't enter 1)* and concentrations taken to the zero power do not appear.
**Rate =** [Text box]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc0168238-e244-4a34-84ac-e572ee66fc4c%2Fb5450d95-4b0c-487f-a40a-bfbf72484767%2F4hafa12_processed.png&w=3840&q=75)
Transcribed Image Text:**The reaction for the formation of phosgene from carbon monoxide and chlorine**
\[ \text{CO} + \text{Cl}_2 \longrightarrow \text{COCl}_2 \]
is first order in CO and second order overall.
**Complete the rate law for this reaction in the box below.**
Use the form k[A]^m[B]^n..., where '1' is understood for m, n... *(don't enter 1)* and concentrations taken to the zero power do not appear.
**Rate =** [Text box]
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