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A student ran the following reaction in the laboratory at 656 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 8.62×10-2 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 0.118 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = ?

A student ran the following reaction in the laboratory at 656 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 8.62×10-2 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 0.118 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = ?

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
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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A student ran the following reaction in the laboratory at 656 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 8.62×10-2 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 0.118 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = ?

 

 

A student ran the following reaction in the laboratory at 656 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 8.62×10-2 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 0.118 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = ?
Transcribed Image Text:A student ran the following reaction in the laboratory at 656 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 8.62×10-2 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 0.118 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = ?
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