Consider the following system at equilibrium where AH° = -198 kJ, and K. = 34.5, at 1150 K. %3D %3D 250-(g) + O2(g) 2503(g) When 0.29 moles of O2(g) are removed from the equilibrium system at constant temperature: The value of K. (remains the same. : The value of Q[ is greater than JKc- The reaction must run in the forward direction to restablish equilibrium. o run in the reverse direction to restablish equilibrium. oremain the same. It is already at equilibrium. The concentration of SO2 will ( decrease.
Consider the following system at equilibrium where AH° = -198 kJ, and K. = 34.5, at 1150 K. %3D %3D 250-(g) + O2(g) 2503(g) When 0.29 moles of O2(g) are removed from the equilibrium system at constant temperature: The value of K. (remains the same. : The value of Q[ is greater than JKc- The reaction must run in the forward direction to restablish equilibrium. o run in the reverse direction to restablish equilibrium. oremain the same. It is already at equilibrium. The concentration of SO2 will ( decrease.
Chemistry
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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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![### Chemical Equilibrium Problem
**Consider the following system at equilibrium where ΔH° = -198 kJ, and Kₒ = 34.5, at 1150 K.**
\[ 2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) \]
When **0.29 moles of O₂(g)** are **removed** from the equilibrium system at constant temperature:
1. **The value of Kₒ:**
- **remains the same.** (Dropdown Selection)
2. **The value of Qₒ:**
- **is greater than** Kₒ. (Dropdown Selection)
3. **The reaction must:**
- **run in the reverse direction to reestablish equilibrium.** (Radio Button Selection)
4. **The concentration of SO₂ will:**
- **decrease.** (Dropdown Selection)
#### Explanation:
1. **Equilibrium Constant (Kᶜ):**
- Kᶜ is a constant for a given temperature, so removing O₂ does not change the value of Kᶜ. It remains the same.
2. **Reaction Quotient (Qᶜ):**
- The reaction quotient Qᶜ is used to determine the direction the reaction must proceed to return to equilibrium. When O₂ is removed, Qᶜ becomes greater than Kᶜ, indicating that the system is no longer at equilibrium.
3. **Direction to Reestablish Equilibrium:**
- When Qᶜ > Kᶜ, the reaction must shift in the reverse direction (towards reactants) to reestablish equilibrium.
4. **Concentration of SO₂:**
- To counter the removal of O₂ and shift the reaction towards the reactants, the concentration of SO₂ will decrease as the equilibrium reestablishes itself.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbc7db68c-7828-4a06-bc34-18cdd71bf49b%2F58321ef9-2670-4d12-a83f-338dec0a7cc8%2Fb54pj5i_processed.png&w=3840&q=75)
Transcribed Image Text:### Chemical Equilibrium Problem
**Consider the following system at equilibrium where ΔH° = -198 kJ, and Kₒ = 34.5, at 1150 K.**
\[ 2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) \]
When **0.29 moles of O₂(g)** are **removed** from the equilibrium system at constant temperature:
1. **The value of Kₒ:**
- **remains the same.** (Dropdown Selection)
2. **The value of Qₒ:**
- **is greater than** Kₒ. (Dropdown Selection)
3. **The reaction must:**
- **run in the reverse direction to reestablish equilibrium.** (Radio Button Selection)
4. **The concentration of SO₂ will:**
- **decrease.** (Dropdown Selection)
#### Explanation:
1. **Equilibrium Constant (Kᶜ):**
- Kᶜ is a constant for a given temperature, so removing O₂ does not change the value of Kᶜ. It remains the same.
2. **Reaction Quotient (Qᶜ):**
- The reaction quotient Qᶜ is used to determine the direction the reaction must proceed to return to equilibrium. When O₂ is removed, Qᶜ becomes greater than Kᶜ, indicating that the system is no longer at equilibrium.
3. **Direction to Reestablish Equilibrium:**
- When Qᶜ > Kᶜ, the reaction must shift in the reverse direction (towards reactants) to reestablish equilibrium.
4. **Concentration of SO₂:**
- To counter the removal of O₂ and shift the reaction towards the reactants, the concentration of SO₂ will decrease as the equilibrium reestablishes itself.
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