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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
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
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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.
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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