Sulfur dioxide and oxygen react to form sulfur trioxide, like this: 2 SO2(9) + O2(9) → 2 SO3(9) Also, a chemist finds that at a certain temperature the equilibrium mixture of sulfur dioxide, oxygen, and sulfur tr has the following composition: compound pressure at equilibrium SO, 40.5 atm O2 39.3 atm SO3 71.0 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0
Sulfur dioxide and oxygen react to form sulfur trioxide, like this: 2 SO2(9) + O2(9) → 2 SO3(9) Also, a chemist finds that at a certain temperature the equilibrium mixture of sulfur dioxide, oxygen, and sulfur tr has the following composition: compound pressure at equilibrium SO, 40.5 atm O2 39.3 atm SO3 71.0 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![### Equilibrium Reaction of Sulfur Dioxide and Oxygen to Form Sulfur Trioxide
When sulfur dioxide (\( \text{SO}_2 \)) and oxygen (\( \text{O}_2 \)) react, they form sulfur trioxide (\( \text{SO}_3 \)) as shown in the chemical equation:
\[ 2 \, \text{SO}_2(g) + \text{O}_2(g) \rightarrow 2 \, \text{SO}_3(g) \]
At a certain temperature, a chemist observed the following equilibrium pressures of the involved gases:
| Compound | Pressure at Equilibrium (atm) |
|----------|-------------------------------|
| \( \text{SO}_2 \) | 40.5 |
| \( \text{O}_2 \) | 39.3 |
| \( \text{SO}_3 \) | 71.0 |
### Calculation of the Equilibrium Constant (\( K_p \))
The equilibrium constant \( K_p \) for this reaction can be calculated using the partial pressures of the gases at equilibrium. To find \( K_p \), use the equation:
\[ K_p = \frac{{(\text{Pressure of } \, \text{SO}_3)^2}}{{(\text{Pressure of } \, \text{SO}_2)^2 \times (\text{Pressure of } \, \text{O}_2)}} \]
Substitute the given pressures into the equation:
\[ K_p = \frac{{(71.0)^2}}{{(40.5)^2 \times (39.3)}} \]
Finally, calculate and round your answer to two significant digits.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1e77a53e-015e-4d74-8706-0af5e82649c9%2F6982dfd9-0703-4724-9628-9a66a12ed0ae%2Fat175h_processed.png&w=3840&q=75)
Transcribed Image Text:### Equilibrium Reaction of Sulfur Dioxide and Oxygen to Form Sulfur Trioxide
When sulfur dioxide (\( \text{SO}_2 \)) and oxygen (\( \text{O}_2 \)) react, they form sulfur trioxide (\( \text{SO}_3 \)) as shown in the chemical equation:
\[ 2 \, \text{SO}_2(g) + \text{O}_2(g) \rightarrow 2 \, \text{SO}_3(g) \]
At a certain temperature, a chemist observed the following equilibrium pressures of the involved gases:
| Compound | Pressure at Equilibrium (atm) |
|----------|-------------------------------|
| \( \text{SO}_2 \) | 40.5 |
| \( \text{O}_2 \) | 39.3 |
| \( \text{SO}_3 \) | 71.0 |
### Calculation of the Equilibrium Constant (\( K_p \))
The equilibrium constant \( K_p \) for this reaction can be calculated using the partial pressures of the gases at equilibrium. To find \( K_p \), use the equation:
\[ K_p = \frac{{(\text{Pressure of } \, \text{SO}_3)^2}}{{(\text{Pressure of } \, \text{SO}_2)^2 \times (\text{Pressure of } \, \text{O}_2)}} \]
Substitute the given pressures into the equation:
\[ K_p = \frac{{(71.0)^2}}{{(40.5)^2 \times (39.3)}} \]
Finally, calculate and round your answer to two significant digits.
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