The following reaction was followed by the method of initial rates: 5 Br (aq) + BrO3¯(aq) + H*(aq) →→→ 3 Br₂(aq) + 3 H₂O(/) with the following results. Exp I II III IV [Br] [BrO3¯ ] 0.10 0.15 0.10 0.10 0.10 0.10 0.20 0.10 What are the units of the rate constant? O M-²5-2 O M-²5-1 O M-³5-1 OM-³5-2 H+ 0.10 0.10 0.10 0.25 (A[BrO3 ]/At)o M.S-1 6.8 x 10-4 1.0 x 10-3 1.4 x 10-3 4.3 x 10-3³ What is the rate law for the reaction? (Example input 'rate = k. [A]^2 . [B]'.) What is the value of the rate constant at the temperature of the experiments? 4.0

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
100%
### Chemical Reaction Kinetics: Initial Rates Method

The following reaction was studied using the method of initial rates:

\[ 
5 \, \text{Br}^-(\text{aq}) + \text{BrO}_3^-(\text{aq}) + \text{H}^+(\text{aq}) \rightarrow 3 \, \text{Br}_2(\text{aq}) + 3 \, \text{H}_2\text{O}(l) 
\]

The table below shows the experimental results:

| Experiment | [Br\(^-\)]\(_0\) (M) | [BrO\(_3^-\)] (M) | [H\(^+\)] (M) | \((\Delta[\text{BrO}_3^-]/\Delta t)_0\) \((\text{M s}^{-1})\) |
|:----------:|:------------------:|:----------------:|:-------------:|:----------------------------------:|
| I          | 0.10               | 0.10             | 0.10          | \(6.8 \times 10^{-4}\)              |
| II         | 0.15               | 0.10             | 0.10          | \(1.0 \times 10^{-3}\)              |
| III        | 0.10               | 0.20             | 0.10          | \(1.4 \times 10^{-3}\)              |
| IV         | 0.10               | 0.10             | 0.25          | \(4.3 \times 10^{-3}\)              |

### Questions:

1. **What is the rate law for the reaction?**
   - Example input: `rate = k . [A]^2 . [B]`.

2. **What is the value of the rate constant at the temperature of the experiments?**
   - Input box provided for numerical answer.

3. **What are the units of the rate constant?**
   - Options:
     - \( \text{M}^{-2}\text{s}^{-2} \)
     - \( \text{M}^{-2} \text{s}^{-1} \)
     - \( \text{M}^{-3} \text{s}^{-1} \)
     - \( \text
Transcribed Image Text:### Chemical Reaction Kinetics: Initial Rates Method The following reaction was studied using the method of initial rates: \[ 5 \, \text{Br}^-(\text{aq}) + \text{BrO}_3^-(\text{aq}) + \text{H}^+(\text{aq}) \rightarrow 3 \, \text{Br}_2(\text{aq}) + 3 \, \text{H}_2\text{O}(l) \] The table below shows the experimental results: | Experiment | [Br\(^-\)]\(_0\) (M) | [BrO\(_3^-\)] (M) | [H\(^+\)] (M) | \((\Delta[\text{BrO}_3^-]/\Delta t)_0\) \((\text{M s}^{-1})\) | |:----------:|:------------------:|:----------------:|:-------------:|:----------------------------------:| | I | 0.10 | 0.10 | 0.10 | \(6.8 \times 10^{-4}\) | | II | 0.15 | 0.10 | 0.10 | \(1.0 \times 10^{-3}\) | | III | 0.10 | 0.20 | 0.10 | \(1.4 \times 10^{-3}\) | | IV | 0.10 | 0.10 | 0.25 | \(4.3 \times 10^{-3}\) | ### Questions: 1. **What is the rate law for the reaction?** - Example input: `rate = k . [A]^2 . [B]`. 2. **What is the value of the rate constant at the temperature of the experiments?** - Input box provided for numerical answer. 3. **What are the units of the rate constant?** - Options: - \( \text{M}^{-2}\text{s}^{-2} \) - \( \text{M}^{-2} \text{s}^{-1} \) - \( \text{M}^{-3} \text{s}^{-1} \) - \( \text
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 9 steps with 1 images

Blurred answer
Knowledge Booster
Rate Laws
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
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