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At a certain temperature, 0.4811 mol of N₂ and 1.701 mol of H₂ are placed in a 5.00 L container. N₂(g) + 3 H₂(g) = 2 NH3(g) At equilibrium, 0.1601 mol of N₂ is present. Calculate the equilibrium constant, Kc. Kc = 89.34 Incorrect

At a certain temperature, 0.4811 mol of N₂ and 1.701 mol of H₂ are placed in a 5.00 L container. N₂(g) + 3 H₂(g) = 2 NH3(g) At equilibrium, 0.1601 mol of N₂ is present. Calculate the equilibrium constant, Kc. Kc = 89.34 Incorrect

World of Chemistry, 3rd edition
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 17A
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At a certain temperature, 0.4811 mol of N₂ and 1.701 mol of H₂ are placed in a 5.00 L container. 2 N₂(g) + 3 H₂(g) = 2NH₂(g) At equilibrium, 0.1601 mol of N₂ is present. Calculate the equilibrium constant, Kỵ. Kc 89.34 Incorrect
Transcribed Image Text:At a certain temperature, 0.4811 mol of N₂ and 1.701 mol of H₂ are placed in a 5.00 L container. 2 N₂(g) + 3 H₂(g) = 2NH₂(g) At equilibrium, 0.1601 mol of N₂ is present. Calculate the equilibrium constant, Kỵ. Kc 89.34 Incorrect
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