Given the following reaction: 2S02(g) + 02(g) = 2S03(g) A mixture of SO2 and 02 was maintained at 800K until the system reached equilibrium. The equilibrium mixture contained 5.0 x 10-2 M SO3, 3.5 x 10-3 M O2, and 3.0 x 10-3 M SO2. Calculate Kat this temperature.
Given the following reaction: 2S02(g) + 02(g) = 2S03(g) A mixture of SO2 and 02 was maintained at 800K until the system reached equilibrium. The equilibrium mixture contained 5.0 x 10-2 M SO3, 3.5 x 10-3 M O2, and 3.0 x 10-3 M SO2. Calculate Kat this temperature.
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Chapter1: Chemical Foundations
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![### Chemical Equilibrium Calculation
**Given the following reaction:**
\[ 2\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightleftharpoons 2\text{SO}_3(\text{g}) \]
A mixture of \(\text{SO}_2\) and \(\text{O}_2\) was maintained at 800 K until the system reached equilibrium. The equilibrium mixture contained \(5.0 \times 10^{-2}\) M \(\text{SO}_3\), \(3.5 \times 10^{-3}\) M \(\text{O}_2\), and \(3.0 \times 10^{-3}\) M \(\text{SO}_2\). Calculate the equilibrium constant \(K\) at this temperature.
**Explanation:**
- **Reactants:** Sulfur dioxide (\(\text{SO}_2\)) and Oxygen (\(\text{O}_2\))
- **Products:** Sulfur trioxide (\(\text{SO}_3\))
- **Conditions:** The reaction is conducted at 800 K.
**Equilibrium Concentrations:**
- \([\text{SO}_3]\) = \(5.0 \times 10^{-2}\) M
- \([\text{O}_2]\) = \(3.5 \times 10^{-3}\) M
- \([\text{SO}_2]\) = \(3.0 \times 10^{-3}\) M
**Required Calculation:**
- Calculate the equilibrium constant \(K\).
To calculate the equilibrium constant \(K\), use the expression for the equilibrium constant for the given balanced chemical reaction.
\[ K = \frac{[\text{SO}_3]^2}{[\text{SO}_2]^2 [\text{O}_2]} \]
By substituting the equilibrium concentrations in the equilibrium expression, \(K\) can be calculated.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F560885b1-95a6-46a1-8479-9132da42c8bd%2F558abcf4-9173-4594-abf7-d3f996814a59%2F83oukh5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Equilibrium Calculation
**Given the following reaction:**
\[ 2\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightleftharpoons 2\text{SO}_3(\text{g}) \]
A mixture of \(\text{SO}_2\) and \(\text{O}_2\) was maintained at 800 K until the system reached equilibrium. The equilibrium mixture contained \(5.0 \times 10^{-2}\) M \(\text{SO}_3\), \(3.5 \times 10^{-3}\) M \(\text{O}_2\), and \(3.0 \times 10^{-3}\) M \(\text{SO}_2\). Calculate the equilibrium constant \(K\) at this temperature.
**Explanation:**
- **Reactants:** Sulfur dioxide (\(\text{SO}_2\)) and Oxygen (\(\text{O}_2\))
- **Products:** Sulfur trioxide (\(\text{SO}_3\))
- **Conditions:** The reaction is conducted at 800 K.
**Equilibrium Concentrations:**
- \([\text{SO}_3]\) = \(5.0 \times 10^{-2}\) M
- \([\text{O}_2]\) = \(3.5 \times 10^{-3}\) M
- \([\text{SO}_2]\) = \(3.0 \times 10^{-3}\) M
**Required Calculation:**
- Calculate the equilibrium constant \(K\).
To calculate the equilibrium constant \(K\), use the expression for the equilibrium constant for the given balanced chemical reaction.
\[ K = \frac{[\text{SO}_3]^2}{[\text{SO}_2]^2 [\text{O}_2]} \]
By substituting the equilibrium concentrations in the equilibrium expression, \(K\) can be calculated.
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