Hydrogen bromide and oxygen react to form bromine and water, like this: 4 HBr(g) + 0₂(g) →2 Br₂(g) + 2H₂O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen bromide, oxygen, bromine, and water has the following composition: compound concentration at equilibrium HBr 1.3 M 0₂ 1.9M Br₂ 0.18M H₂O 0.73 M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits.
Hydrogen bromide and oxygen react to form bromine and water, like this: 4 HBr(g) + 0₂(g) →2 Br₂(g) + 2H₂O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen bromide, oxygen, bromine, and water has the following composition: compound concentration at equilibrium HBr 1.3 M 0₂ 1.9M Br₂ 0.18M H₂O 0.73 M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![**Reaction and Equilibrium Constant Calculation**
In a chemical reaction, **hydrogen bromide** and **oxygen** react to form **bromine** and **water**, as shown in the equation below:
\[ 4 \text{HBr}(g) + \text{O}_2(g) \rightarrow 2 \text{Br}_2(g) + 2 \text{H}_2\text{O}(g) \]
A chemist observes that at a specific temperature, the equilibrium mixture contains the following concentrations:
| Compound | Concentration at Equilibrium |
|-----------|-------------------------------|
| HBr | 1.3 M |
| O₂ | 1.9 M |
| Br₂ | 0.18 M |
| H₂O | 0.73 M |
**Task:** Calculate the equilibrium constant \( K_c \) for this reaction. Round your answer to two significant digits.
**Equation for \( K_c \):**
The expression for the equilibrium constant \( K_c \) is derived from the balanced chemical equation:
\[ K_c = \frac{[\text{Br}_2]^2[\text{H}_2O]^2}{[\text{HBr}]^4 [\text{O}_2]} \]
Use the concentrations provided to calculate \( K_c \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F868a7cc3-2ad7-4fe7-9a39-259d78c013d4%2Fb5d94200-921e-47f7-bb7f-4582c703281d%2F2mndytv_processed.png&w=3840&q=75)
Transcribed Image Text:**Reaction and Equilibrium Constant Calculation**
In a chemical reaction, **hydrogen bromide** and **oxygen** react to form **bromine** and **water**, as shown in the equation below:
\[ 4 \text{HBr}(g) + \text{O}_2(g) \rightarrow 2 \text{Br}_2(g) + 2 \text{H}_2\text{O}(g) \]
A chemist observes that at a specific temperature, the equilibrium mixture contains the following concentrations:
| Compound | Concentration at Equilibrium |
|-----------|-------------------------------|
| HBr | 1.3 M |
| O₂ | 1.9 M |
| Br₂ | 0.18 M |
| H₂O | 0.73 M |
**Task:** Calculate the equilibrium constant \( K_c \) for this reaction. Round your answer to two significant digits.
**Equation for \( K_c \):**
The expression for the equilibrium constant \( K_c \) is derived from the balanced chemical equation:
\[ K_c = \frac{[\text{Br}_2]^2[\text{H}_2O]^2}{[\text{HBr}]^4 [\text{O}_2]} \]
Use the concentrations provided to calculate \( K_c \).
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