Sulfur dioxide reacts with carbon dioxide to form an equilibrium with sulfur trioxide and carbon monoxide, all gases (see the reaction below). A mixture of 1.91 mole each of sulfur dioxide and carbon dioxide is placed in an 2.9 L container and allowed to reach equilibrium. If the equilibrium constant, Kc, is 2.83 at this temperature, what is the concentration of sulfur trioxide at equilibrium? SO₂ (g) + CO₂ (g) = SO3 (g) + CO (g) Keep extra significant figures during the calculation and round your answer to 2 decimal places. This may not be the correct number of significant figures, but do it anyway.
Sulfur dioxide reacts with carbon dioxide to form an equilibrium with sulfur trioxide and carbon monoxide, all gases (see the reaction below). A mixture of 1.91 mole each of sulfur dioxide and carbon dioxide is placed in an 2.9 L container and allowed to reach equilibrium. If the equilibrium constant, Kc, is 2.83 at this temperature, what is the concentration of sulfur trioxide at equilibrium? SO₂ (g) + CO₂ (g) = SO3 (g) + CO (g) Keep extra significant figures during the calculation and round your answer to 2 decimal places. This may not be the correct number of significant figures, but do it anyway.
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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![**Chemical Equilibrium and Concentration Calculation**
Sulfur dioxide reacts with carbon dioxide to form an equilibrium with sulfur trioxide and carbon monoxide, all gases (see the reaction below). A mixture of 1.91 moles each of sulfur dioxide and carbon dioxide is placed in a 2.9-liter container and allowed to reach equilibrium. If the equilibrium constant, Kc, is 2.83 at this temperature, what is the concentration of sulfur trioxide at equilibrium?
\[ \text{SO}_2 \, (g) + \text{CO}_2 \, (g) \rightleftharpoons \text{SO}_3 \, (g) + \text{CO} \, (g) \]
**Solution Approach:**
1. **Initial Moles and Concentrations**:
- Initial moles of SO2 = 1.91 moles
- Initial moles of CO2 = 1.91 moles
- Volume of the container = 2.9 L
Initial concentrations:
\[ [\text{SO}_2]_0 = \frac{1.91 \, \text{moles}}{2.9 \, \text{L}} \]
\[ [\text{CO}_2]_0 = \frac{1.91 \, \text{moles}}{2.9 \, \text{L}} \]
2. **Setting Up the ICE Table**:
- I (Initial): Concentrations before the reaction starts.
- C (Change): Change in concentrations as the system moves to equilibrium.
- E (Equilibrium): Concentrations when the system reaches equilibrium.
| Species | Initial (M) | Change (M) | Equilibrium (M) |
| ------------|-------------------------|------------|--------------------------|
| SO2 | 0.659 | -x | 0.659 - x |
| CO2 | 0.659 | -x | 0.659 - x |
| SO3 | 0 | +x | x |
| CO | 0 | +x | x |
3. **Equilibrium Expression**:
\[ K_c = \frac{[\text{SO}_3][\text{CO}]}{[\text{](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2cfc3a1d-71f5-4849-9f61-cac9f1c46434%2F425d4898-ba91-4868-bc0f-bec2fb3be749%2Ffu5kicy_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Equilibrium and Concentration Calculation**
Sulfur dioxide reacts with carbon dioxide to form an equilibrium with sulfur trioxide and carbon monoxide, all gases (see the reaction below). A mixture of 1.91 moles each of sulfur dioxide and carbon dioxide is placed in a 2.9-liter container and allowed to reach equilibrium. If the equilibrium constant, Kc, is 2.83 at this temperature, what is the concentration of sulfur trioxide at equilibrium?
\[ \text{SO}_2 \, (g) + \text{CO}_2 \, (g) \rightleftharpoons \text{SO}_3 \, (g) + \text{CO} \, (g) \]
**Solution Approach:**
1. **Initial Moles and Concentrations**:
- Initial moles of SO2 = 1.91 moles
- Initial moles of CO2 = 1.91 moles
- Volume of the container = 2.9 L
Initial concentrations:
\[ [\text{SO}_2]_0 = \frac{1.91 \, \text{moles}}{2.9 \, \text{L}} \]
\[ [\text{CO}_2]_0 = \frac{1.91 \, \text{moles}}{2.9 \, \text{L}} \]
2. **Setting Up the ICE Table**:
- I (Initial): Concentrations before the reaction starts.
- C (Change): Change in concentrations as the system moves to equilibrium.
- E (Equilibrium): Concentrations when the system reaches equilibrium.
| Species | Initial (M) | Change (M) | Equilibrium (M) |
| ------------|-------------------------|------------|--------------------------|
| SO2 | 0.659 | -x | 0.659 - x |
| CO2 | 0.659 | -x | 0.659 - x |
| SO3 | 0 | +x | x |
| CO | 0 | +x | x |
3. **Equilibrium Expression**:
\[ K_c = \frac{[\text{SO}_3][\text{CO}]}{[\text{
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