Ammonia decomposes to form nitrogen and hydrogen, like this: 2 NH3(g) → N₂(g) + 3H₂(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, nitrogen, and hydrogen has the following composition: compound concentration at equilibrium NH3 1.6M N₂ 0.34 M H₂ 0.53 M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = x10 X 3 ?
Ammonia decomposes to form nitrogen and hydrogen, like this: 2 NH3(g) → N₂(g) + 3H₂(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, nitrogen, and hydrogen has the following composition: compound concentration at equilibrium NH3 1.6M N₂ 0.34 M H₂ 0.53 M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = x10 X 3 ?
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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![### Ammonia Decomposition Reaction
Ammonia decomposes to form nitrogen and hydrogen, as shown in the following chemical equation:
\[ 2\text{NH}_3(g) \rightarrow \text{N}_2(g) + 3\text{H}_2(g) \]
A chemist finds that at a certain temperature, the equilibrium mixture of ammonia, nitrogen, and hydrogen has the following composition:
| **Compound** | **Concentration at Equilibrium** |
|--------------|-------------------------------------|
| \(\text{NH}_3\) | 1.6 M |
| \(\text{N}_2\) | 0.34 M |
| \(\text{H}_2\) | 0.53 M |
Calculate the value of the equilibrium constant \( K_c \) for this reaction. Round your answer to 2 significant digits.
\[ K_c = \]
This problem requires determining the equilibrium constant (\( K_c \)), using the formula:
\[ K_c = \frac{[\text{N}_2][\text{H}_2]^3}{[\text{NH}_3]^2} \]
The concentrations at equilibrium are provided, which can be plugged into the formula to calculate \( K_c \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F20b515c9-5e3a-448e-90a2-ac3b562e1523%2F7f71f950-9f86-444c-a799-f7c7d76488c6%2Ficpgelo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Ammonia Decomposition Reaction
Ammonia decomposes to form nitrogen and hydrogen, as shown in the following chemical equation:
\[ 2\text{NH}_3(g) \rightarrow \text{N}_2(g) + 3\text{H}_2(g) \]
A chemist finds that at a certain temperature, the equilibrium mixture of ammonia, nitrogen, and hydrogen has the following composition:
| **Compound** | **Concentration at Equilibrium** |
|--------------|-------------------------------------|
| \(\text{NH}_3\) | 1.6 M |
| \(\text{N}_2\) | 0.34 M |
| \(\text{H}_2\) | 0.53 M |
Calculate the value of the equilibrium constant \( K_c \) for this reaction. Round your answer to 2 significant digits.
\[ K_c = \]
This problem requires determining the equilibrium constant (\( K_c \)), using the formula:
\[ K_c = \frac{[\text{N}_2][\text{H}_2]^3}{[\text{NH}_3]^2} \]
The concentrations at equilibrium are provided, which can be plugged into the formula to calculate \( K_c \).
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