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The following data were collected for a system at equilibrium at a certain temperature. Calculate the equilibrium constant at this temperature for the reaction. ([H2] = 0.1mol/L; [N2] = 1.1 mol/L; [NH3] = 0.0390 mol.L) 3 H2(g) + N2(g) = 2NH3(g)

The following data were collected for a system at equilibrium at a certain temperature. Calculate the equilibrium constant at this temperature for the reaction. ([H2] = 0.1mol/L; [N2] = 1.1 mol/L; [NH3] = 0.0390 mol.L) 3 H2(g) + N2(g) = 2NH3(g)

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.2QE: Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium...
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The following data were collected for a system at equilibrium at a certain temperature. Calculate the equilibrium constant at this temperature for the reaction. ([H,] = 0.1mol/L; [N,] = 1.1 mol/L; [NH3] = 0.0390 mol.L) 3 H2(g) + N2(g) = 2NH3(g) A K=0.014 B) K=0.14 c) K=4.1 D K=1.4
Transcribed Image Text:The following data were collected for a system at equilibrium at a certain temperature. Calculate the equilibrium constant at this temperature for the reaction. ([H,] = 0.1mol/L; [N,] = 1.1 mol/L; [NH3] = 0.0390 mol.L) 3 H2(g) + N2(g) = 2NH3(g) A K=0.014 B) K=0.14 c) K=4.1 D K=1.4
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