[he kinetics of this reaction were studied at 50.9 °C. The following data were obtained by following Ni(CO)4 concentration over time as the reaction took place. 4.0 6.0 Ni(CO),], M | 0.45 | 0.315844| 0.221683 | 0.109207| 0.053799|| 0.013056 | 0.002224 2.0 10.0 ime, sec 1.0 15.0 20.0 What is the half-life of the reaction, in minutes, at 50.9 °C ?
[he kinetics of this reaction were studied at 50.9 °C. The following data were obtained by following Ni(CO)4 concentration over time as the reaction took place. 4.0 6.0 Ni(CO),], M | 0.45 | 0.315844| 0.221683 | 0.109207| 0.053799|| 0.013056 | 0.002224 2.0 10.0 ime, sec 1.0 15.0 20.0 What is the half-life of the reaction, in minutes, at 50.9 °C ?
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...
Related questions
Question
please see attached
![### Decomposition of Nickel Carbonyl (Ni(CO)₄)
**Reaction:**
\[ \text{Ni(CO)}_4 (\text{g}) \rightarrow \text{Ni (s)} + 4 \text{CO (g)} \]
**Study Overview:**
The kinetics of the decomposition of Nickel Carbonyl (Ni(CO)₄) were studied at a temperature of 50.9 °C. The concentration of Ni(CO)₄ was measured over a series of time intervals to observe the reaction's progress.
**Data Table:**
| Time (sec) | [Ni(CO)₄] (M) |
|------------|:-------------:|
| 1.0 | 0.45 |
| 2.0 | 0.315844 |
| 4.0 | 0.221683 |
| 6.0 | 0.109207 |
| 10.0 | 0.053799 |
| 15.0 | 0.013056 |
| 20.0 | 0.002224 |
**Interpretation of the Data:**
The table shows the concentration of Nickel Carbonyl, Ni(CO)₄, at the specified times in seconds. As time progresses, the concentration of Ni(CO)₄ decreases, indicating the rate at which the reaction is occurring and the compound is decomposing.
**Question:**
What is the half-life of the reaction, in minutes, at 50.9 °C?
**Calculation of Half-Life:**
To determine the half-life, find the time it takes for the concentration of Ni(CO)₄ to decrease to half of its initial concentration. The initial concentration is 0.45 M, so we look for the time at which the concentration reaches 0.225 M.
From the given data:
- At 4.0 sec, [Ni(CO)₄] = 0.221683 M
**Conclusion:**
Therefore, the half-life of the reaction at 50.9 °C is approximately 4.0 seconds. Converting this to minutes:
\[ \text{Half-life} = \frac{4.0 \text{ sec}}{60 \text{ sec/min}} \approx 0.067 \text{ minutes} \]
Thus, the half-life of](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4f7442e5-ed1a-4154-ba5d-4813abad6cff%2F6d26846b-897e-4418-a18e-719524745fe7%2F3bviror.png&w=3840&q=75)
Transcribed Image Text:### Decomposition of Nickel Carbonyl (Ni(CO)₄)
**Reaction:**
\[ \text{Ni(CO)}_4 (\text{g}) \rightarrow \text{Ni (s)} + 4 \text{CO (g)} \]
**Study Overview:**
The kinetics of the decomposition of Nickel Carbonyl (Ni(CO)₄) were studied at a temperature of 50.9 °C. The concentration of Ni(CO)₄ was measured over a series of time intervals to observe the reaction's progress.
**Data Table:**
| Time (sec) | [Ni(CO)₄] (M) |
|------------|:-------------:|
| 1.0 | 0.45 |
| 2.0 | 0.315844 |
| 4.0 | 0.221683 |
| 6.0 | 0.109207 |
| 10.0 | 0.053799 |
| 15.0 | 0.013056 |
| 20.0 | 0.002224 |
**Interpretation of the Data:**
The table shows the concentration of Nickel Carbonyl, Ni(CO)₄, at the specified times in seconds. As time progresses, the concentration of Ni(CO)₄ decreases, indicating the rate at which the reaction is occurring and the compound is decomposing.
**Question:**
What is the half-life of the reaction, in minutes, at 50.9 °C?
**Calculation of Half-Life:**
To determine the half-life, find the time it takes for the concentration of Ni(CO)₄ to decrease to half of its initial concentration. The initial concentration is 0.45 M, so we look for the time at which the concentration reaches 0.225 M.
From the given data:
- At 4.0 sec, [Ni(CO)₄] = 0.221683 M
**Conclusion:**
Therefore, the half-life of the reaction at 50.9 °C is approximately 4.0 seconds. Converting this to minutes:
\[ \text{Half-life} = \frac{4.0 \text{ sec}}{60 \text{ sec/min}} \approx 0.067 \text{ minutes} \]
Thus, the half-life of
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 4 steps with 7 images
Knowledge Booster
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.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY