A student ran the following reaction in the laboratory at 586 K: CO(g) + Cl2(g) COCI,(g) When she introduced 0.376 moles of CO(g) and 0.406 moles of Cl½(g) into a 1.00 liter container, she found the equilibrium concentration of COCI,(g) to be 0.337 М. Calculate the equilibrium constant, K, she obtained for this reaction. K =
A student ran the following reaction in the laboratory at 586 K: CO(g) + Cl2(g) COCI,(g) When she introduced 0.376 moles of CO(g) and 0.406 moles of Cl½(g) into a 1.00 liter container, she found the equilibrium concentration of COCI,(g) to be 0.337 М. Calculate the equilibrium constant, K, she obtained for this reaction. K =
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
![### Reaction Equilibrium Calculation at 586 K
A student conducted an experiment to study the following reaction at a temperature of 586 K:
\[ \text{CO(g)} + \text{Cl}_2\text{(g)} \rightleftharpoons \text{COCl}_2\text{(g)} \]
#### Initial Conditions
- **Moles of CO(g)**: 0.376 moles
- **Moles of Cl₂(g)**: 0.406 moles
- **Volume of container**: 1.00 liter
#### Observed Equilibrium Condition
- **Equilibrium concentration of COCl₂(g)**: 0.337 M
#### Calculation of Equilibrium Constant \( K_c \)
To find the equilibrium constant \( K_c \), we need to set up the reaction table and expressions for equilibrium concentrations and then apply the equilibrium constant formula.
1. **Initial Concentrations (in Moles per Liter):**
- \([ \text{CO} ]_0 = \frac{0.376 \text{ moles}}{1.00 \text{ L}} = 0.376 \text{ M}\)
- \([ \text{Cl}_2 ]_0 = \frac{0.406 \text{ moles}}{1.00 \text{ L}} = 0.406 \text{ M}\)
2. **Determination of Changes:**
- At equilibrium, \[\text{COCl}_2 \text{(g)} = 0.337 \text{ M}\]
- Assuming \(x\) moles of CO and \(x\) moles of Cl₂ react to form 0.337 M of the product, then:
- \([ \text{CO} ] = 0.376\text{ M} - x\]
- \([ \text{Cl}_2 ] = 0.406\text{ M} - x\]
- \([ \text{COCl}_2 ] = 0.337 \text{ M}\)
- Since \(x = 0.337 \text{ M}\), the remaining concentrations are:
- \([ \text{CO} ] = 0.376\text{ M} - 0.337\text{ M} = 0.039 \text{ M}\)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9cce6311-c94c-4650-90f7-705d2febbb40%2F2cb25026-10f7-44f6-b25e-3da682a00a37%2Foiqlsx_processed.png&w=3840&q=75)
Transcribed Image Text:### Reaction Equilibrium Calculation at 586 K
A student conducted an experiment to study the following reaction at a temperature of 586 K:
\[ \text{CO(g)} + \text{Cl}_2\text{(g)} \rightleftharpoons \text{COCl}_2\text{(g)} \]
#### Initial Conditions
- **Moles of CO(g)**: 0.376 moles
- **Moles of Cl₂(g)**: 0.406 moles
- **Volume of container**: 1.00 liter
#### Observed Equilibrium Condition
- **Equilibrium concentration of COCl₂(g)**: 0.337 M
#### Calculation of Equilibrium Constant \( K_c \)
To find the equilibrium constant \( K_c \), we need to set up the reaction table and expressions for equilibrium concentrations and then apply the equilibrium constant formula.
1. **Initial Concentrations (in Moles per Liter):**
- \([ \text{CO} ]_0 = \frac{0.376 \text{ moles}}{1.00 \text{ L}} = 0.376 \text{ M}\)
- \([ \text{Cl}_2 ]_0 = \frac{0.406 \text{ moles}}{1.00 \text{ L}} = 0.406 \text{ M}\)
2. **Determination of Changes:**
- At equilibrium, \[\text{COCl}_2 \text{(g)} = 0.337 \text{ M}\]
- Assuming \(x\) moles of CO and \(x\) moles of Cl₂ react to form 0.337 M of the product, then:
- \([ \text{CO} ] = 0.376\text{ M} - x\]
- \([ \text{Cl}_2 ] = 0.406\text{ M} - x\]
- \([ \text{COCl}_2 ] = 0.337 \text{ M}\)
- Since \(x = 0.337 \text{ M}\), the remaining concentrations are:
- \([ \text{CO} ] = 0.376\text{ M} - 0.337\text{ M} = 0.039 \text{ M}\)
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps with 1 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
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](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY