**Consider the following system at equilibrium where \(\Delta H^\circ = -87.9 \, \text{kJ}\), and \(K_c = 83.3\), at \(5.00 \times 10^2 \, \text{K}\):**\[ \text{PCl}_3(g) + \text{Cl}_2(g) \rightleftharpoons \text{PCl}_5(g) \]**If the temperature on the equilibrium system is suddenly decreased:**1. **The value of \(K_c\)** - ○ increases - ○ decreases - ○ remains the same2. **The value of \(Q_c\)** - ○ is less than \(K_c\) - ○ is greater than \(K_c\) - ○ is equal to \(K_c\)3. **The reaction must** - ○ run in the forward direction to reestablish equilibrium - ○ run in the reverse direction to reestablish equilibrium - ○ remain in the current position, since it is already at equilibrium4. **The concentration of \(\text{Cl}_2\) will** - ○ increase - ○ decrease - ○ remain the same

Answer:When QC=KC, reaction mixture is at equilibrium.When QC>KC, reaction mixture is not at…

Answered: Consider the following system at…

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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**Consider the following system at equilibrium where \(\Delta H^\circ = -87.9 \, \text{kJ}\), and \(K_c = 83.3\), at \(5.00 \times 10^2 \, \text{K}\):**

\[ \text{PCl}_3(g) + \text{Cl}_2(g) \rightleftharpoons \text{PCl}_5(g) \]

**If the temperature on the equilibrium system is suddenly decreased:**

1. **The value of \(K_c\)**
- ○ increases
- ○ decreases
- ○ remains the same

2. **The value of \(Q_c\)**
- ○ is less than \(K_c\)
- ○ is greater than \(K_c\)
- ○ is equal to \(K_c\)

3. **The reaction must**
- ○ run in the forward direction to reestablish equilibrium
- ○ run in the reverse direction to reestablish equilibrium
- ○ remain in the current position, since it is already at equilibrium

4. **The concentration of \(\text{Cl}_2\) will**
- ○ increase
- ○ decrease
- ○ remain the same

Expert Solution

Step 1: Relation between reaction quotient and equilibrium constant

Answer:

When Q_C=K_C, reaction mixture is at equilibrium.
When Q_C>K_C, reaction mixture is not at equilibrium and reaction has to move in reverse direction, so that value of Q_C can decrease and become equal to K_C and system can be at equilibrium again.
When Q_C<K_C, reaction mixture is not at equilibrium and reaction has to move in forward direction, so that value of Q_C can increase and become equal to K_C and system can be at equilibrium again.

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