At a certain temperature, 0.3811 mol of N₂ and 1.761 mol of H₂ are placed in a 4.50 L container according to the following equation: N₂(g) + 3H₂(g) + 2NH3(g) At equilibrium, 0.1001mol of N2 is present. Calculate the equilibrium constant.
At a certain temperature, 0.3811 mol of N₂ and 1.761 mol of H₂ are placed in a 4.50 L container according to the following equation: N₂(g) + 3H₂(g) + 2NH3(g) At equilibrium, 0.1001mol of N2 is present. Calculate the equilibrium constant.
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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![At a certain temperature, 0.3811 mol of \( \text{N}_2 \) and 1.761 mol of \( \text{H}_2 \) are placed in a 4.50 L container according to the following equation:
\[ \text{N}_2(g) + 3\text{H}_2(g) \leftrightarrow 2\text{NH}_3(g) \]
At equilibrium, 0.1001 mol of \( \text{N}_2 \) is present. Calculate the equilibrium constant.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F078de29d-732f-4e63-accc-2adc1016c930%2Ff755da8f-9a72-42b9-8f91-6f919493ff5c%2Fot9wfhy_processed.jpeg&w=3840&q=75)
Transcribed Image Text:At a certain temperature, 0.3811 mol of \( \text{N}_2 \) and 1.761 mol of \( \text{H}_2 \) are placed in a 4.50 L container according to the following equation:
\[ \text{N}_2(g) + 3\text{H}_2(g) \leftrightarrow 2\text{NH}_3(g) \]
At equilibrium, 0.1001 mol of \( \text{N}_2 \) is present. Calculate the equilibrium constant.
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Equilibrium constant of a reaction is an expression that shows relationship between reactants and products of a chemical reaction at equilibrium.
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