The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH, + NO, N2 + 2 H,0 Experiment NH, Jo. M [NO2], M Initial Rate, Ms1 9.44x10-6 1.89x10-5 1.89×10-5 3.79x10-5 1 0.212 0.146 2 0.212 0.293 3 0.424 0.146 4 0.424 0.293 Complete the rate law for this reaction in the box below. Use the form k[A]|B}", where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is

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...
icon
Related questions
Question
The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution:

\[
\text{NH}_4^+ + \text{NO}_2^- \rightarrow \text{N}_2 + 2 \text{H}_2\text{O}
\]

| Experiment | \([\text{NH}_4^+]_0\) M | \([\text{NO}_2^-]_0\) M | Initial Rate, M/s |
|------------|------------------|------------------|---------------------|
| 1          | 0.212            | 0.146            | \(9.44 \times 10^{-6}\)  |
| 2          | 0.212            | 0.293            | \(1.89 \times 10^{-5}\)  |
| 3          | 0.424            | 0.146            | \(1.89 \times 10^{-5}\)  |
| 4          | 0.424            | 0.293            | \(3.79 \times 10^{-5}\)  |

**Complete the rate law for this reaction in the box below.**  
Use the form \(k[\text{A}]^m[\text{B}]^n\), where '1' is understood for m or n and concentrations taken to the zero power do not appear.  
*Don't enter 1 for m or n*

Rate = \_\_\_\_\_\_

From these data, the rate constant is \_\_\_\_\_\_ M\(^1\), \(\text{s}^{-1}\).
Transcribed Image Text:The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: \[ \text{NH}_4^+ + \text{NO}_2^- \rightarrow \text{N}_2 + 2 \text{H}_2\text{O} \] | Experiment | \([\text{NH}_4^+]_0\) M | \([\text{NO}_2^-]_0\) M | Initial Rate, M/s | |------------|------------------|------------------|---------------------| | 1 | 0.212 | 0.146 | \(9.44 \times 10^{-6}\) | | 2 | 0.212 | 0.293 | \(1.89 \times 10^{-5}\) | | 3 | 0.424 | 0.146 | \(1.89 \times 10^{-5}\) | | 4 | 0.424 | 0.293 | \(3.79 \times 10^{-5}\) | **Complete the rate law for this reaction in the box below.** Use the form \(k[\text{A}]^m[\text{B}]^n\), where '1' is understood for m or n and concentrations taken to the zero power do not appear. *Don't enter 1 for m or n* Rate = \_\_\_\_\_\_ From these data, the rate constant is \_\_\_\_\_\_ M\(^1\), \(\text{s}^{-1}\).
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 3 images

Blurred answer
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY