R eq req freq [Review Topics] [References) Use the References to access important values if needed for this question. Consider the following reaction where Ke = 77.5 at 600 K. CO(g) + Cl₂(g) CoCl₂(g) A reaction mixture was found to contain 4.23x10-2 moles of CO(g), 4.00x10-2 moles of Cl₂(g) and 0.105 moles of CoCl₂(g), In a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals SAVAGE X FENTY... The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. Is at equilibrium. 20
R eq req freq [Review Topics] [References) Use the References to access important values if needed for this question. Consider the following reaction where Ke = 77.5 at 600 K. CO(g) + Cl₂(g) CoCl₂(g) A reaction mixture was found to contain 4.23x10-2 moles of CO(g), 4.00x10-2 moles of Cl₂(g) and 0.105 moles of CoCl₂(g), In a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals SAVAGE X FENTY... The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. Is at equilibrium. 20
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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Question
![## Equilibrium Reaction Study
**Reaction Details:**
- Consider the following reaction where \( K_c = 77.5 \) at 600 K.
\[
\text{CO(g) + Cl}_2\text{(g) } \rightleftharpoons \text{ COCl}_2\text{(g)}
\]
**Reaction Mixture Information:**
- A reaction mixture was found to contain:
- 4.23 x 10\(^{-2}\) moles of CO(g)
- 4.00 x 10\(^{-2}\) moles of Cl\(_2\)(g)
- 0.105 moles of COCl\(_2\)(g)
in a 1.00 liter container.
**Equilibrium Analysis:**
- **Is the reaction at equilibrium?**
- **If not, what direction must it run in order to reach equilibrium?**
### Calculation
1. **Reaction Quotient (\(Q_c\))**:
- Compare \(Q_c\) to \(K_c\) to determine the necessary direction to reach equilibrium.
2. **Options:**
- A. Must run in the forward direction to reach equilibrium.
- B. Must run in the reverse direction to reach equilibrium.
- C. Is at equilibrium.
**Submit:** Use calculations to find \(Q_c\) and determine the direction.
(Blank section for students to input their answer.)
**Note:**
- Submit your answer and try again if necessary.
**End of Exercise**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3e5f0bee-bbde-421f-8347-e8b63f453811%2F1036188b-ea02-47ee-acc6-69c884fd9e1a%2Fj0uqc2_processed.jpeg&w=3840&q=75)
Transcribed Image Text:## Equilibrium Reaction Study
**Reaction Details:**
- Consider the following reaction where \( K_c = 77.5 \) at 600 K.
\[
\text{CO(g) + Cl}_2\text{(g) } \rightleftharpoons \text{ COCl}_2\text{(g)}
\]
**Reaction Mixture Information:**
- A reaction mixture was found to contain:
- 4.23 x 10\(^{-2}\) moles of CO(g)
- 4.00 x 10\(^{-2}\) moles of Cl\(_2\)(g)
- 0.105 moles of COCl\(_2\)(g)
in a 1.00 liter container.
**Equilibrium Analysis:**
- **Is the reaction at equilibrium?**
- **If not, what direction must it run in order to reach equilibrium?**
### Calculation
1. **Reaction Quotient (\(Q_c\))**:
- Compare \(Q_c\) to \(K_c\) to determine the necessary direction to reach equilibrium.
2. **Options:**
- A. Must run in the forward direction to reach equilibrium.
- B. Must run in the reverse direction to reach equilibrium.
- C. Is at equilibrium.
**Submit:** Use calculations to find \(Q_c\) and determine the direction.
(Blank section for students to input their answer.)
**Note:**
- Submit your answer and try again if necessary.
**End of Exercise**
Expert Solution
Step 1
We know for a reaction to be in equilibrium the reaction quotient must be equal to equilibrium constant .
The only difference between Qc and Kc is that in Kc equilibrium concentration of reactant and product is used .
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