This question has multiple parts. Work The reaction 2NO(g) + Cl₂(g) → 2NOCI(g) was studied at -10°C. The following results were obtained where A[C1₂] At Rate = - [NO]o [C12]o (mol/L) (mol/L) 0.12 0.12 0.12 0.24 0.24 0.24 Initial Rate (mol/L.min) 0.31 0.62 2.49 a What is the rate law? (Use k for the rate constant. ) Rate = K[NO]²[C1₂] Rate constant = What is the value of the rate constant? the parts to get the most points. L² mol². min
This question has multiple parts. Work The reaction 2NO(g) + Cl₂(g) → 2NOCI(g) was studied at -10°C. The following results were obtained where A[C1₂] At Rate = - [NO]o [C12]o (mol/L) (mol/L) 0.12 0.12 0.12 0.24 0.24 0.24 Initial Rate (mol/L.min) 0.31 0.62 2.49 a What is the rate law? (Use k for the rate constant. ) Rate = K[NO]²[C1₂] Rate constant = What is the value of the rate constant? the parts to get the most points. L² mol². min
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
\[ 2\text{NO}(g) + \text{Cl}_2(g) \rightarrow 2\text{NOCl}(g) \]
was studied at -10°C. The following results were obtained where
\[ \text{Rate} = -\frac{\Delta[\text{Cl}_2]}{\Delta t} \]
A table of initial concentrations and rates is presented as follows:
| \([\text{NO}]_0\) (mol/L) | \([\text{Cl}_2]_0\) (mol/L) | Initial Rate (mol/L·min) |
|--------------------------|-----------------------------|-------------------------|
| 0.12 | 0.12 | 0.31 |
| 0.12 | 0.24 | 0.62 |
| 0.24 | 0.24 | 2.49 |
**(a) What is the rate law?**
(Use \( k \) for the rate constant.)
\[ \text{Rate} = k[\text{NO}]^2[\text{Cl}_2] \]
**(b) What is the value of the rate constant?**
The units for the rate constant are \(\frac{L^2}{\text{mol}^2 \cdot \text{min}}\).
[The space for the value is left blank for calculation.]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F216d8975-823a-443e-8abc-06f056adfa09%2Fb9facbc2-8d2e-4da7-9845-7e8ed566f491%2Ffwc1czd_processed.png&w=3840&q=75)
Transcribed Image Text:The reaction
\[ 2\text{NO}(g) + \text{Cl}_2(g) \rightarrow 2\text{NOCl}(g) \]
was studied at -10°C. The following results were obtained where
\[ \text{Rate} = -\frac{\Delta[\text{Cl}_2]}{\Delta t} \]
A table of initial concentrations and rates is presented as follows:
| \([\text{NO}]_0\) (mol/L) | \([\text{Cl}_2]_0\) (mol/L) | Initial Rate (mol/L·min) |
|--------------------------|-----------------------------|-------------------------|
| 0.12 | 0.12 | 0.31 |
| 0.12 | 0.24 | 0.62 |
| 0.24 | 0.24 | 2.49 |
**(a) What is the rate law?**
(Use \( k \) for the rate constant.)
\[ \text{Rate} = k[\text{NO}]^2[\text{Cl}_2] \]
**(b) What is the value of the rate constant?**
The units for the rate constant are \(\frac{L^2}{\text{mol}^2 \cdot \text{min}}\).
[The space for the value is left blank for calculation.]
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