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Initially 1.50 moles of N₂(g) and 3.50 moles of H₂(g) were added to a 1.00 L container at 700 °C. As a result of the reaction, 3H₂(g) + N₂(g) 2NH₂(g) the equilibrium concentration of NH₂(g) became 0.540 M. What is the value of the equilibrium constant for this reaction at 700 °C?

Initially 1.50 moles of N₂(g) and 3.50 moles of H₂(g) were added to a 1.00 L container at 700 °C. As a result of the reaction, 3H₂(g) + N₂(g) 2NH₂(g) the equilibrium concentration of NH₂(g) became 0.540 M. What is the value of the equilibrium constant for this reaction at 700 °C?

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter13: Fundamental Equilibrium Concepts
Section: Chapter Questions
Problem 56E: At 1 atm and 25 C, NO2 with an initial concentration of 1.00 M is 3.3103 decomposed into NO and O2....
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Initially 1.50 moles of N₂(g) and 3.50 moles of H₂(g) were added to a 1.00 L container at 700 °C. As a result of the 2NH₂(g) the equilibrium reaction, 3H₂(g) + N₂(g) concentration of NH₂(g) became 0.540 M. What is the value of the equilibrium constant for this reaction at 700 °C?
Transcribed Image Text:Initially 1.50 moles of N₂(g) and 3.50 moles of H₂(g) were added to a 1.00 L container at 700 °C. As a result of the 2NH₂(g) the equilibrium reaction, 3H₂(g) + N₂(g) concentration of NH₂(g) became 0.540 M. What is the value of the equilibrium constant for this reaction at 700 °C?
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