A student ran the following reaction in the laboratory at 744 K:N2(g) + 3H2(g) 2NH3(g)When she introduced 4.00×10-2 moles of N2(g) and 5.96×10-2 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 8.88×10-4 M.Calculate the equilibrium constant, Kc, she obtained for this reaction. A student ran the following reaction in the laboratory at 744 K:N2(g) + 3H2(g)2NH3(g)When she introduced 4.00x10-2 moles of N2(g) and 5.96×10 2 moles of H2(9) intoa 1.00 liter container, she found the equilibrium concentration of NH3(g) to be8.88x10-4 M.Calculate the equilibrium constant, Ke, she obtained for this reaction.

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Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section15.3: Determining An Equilibrium Constant

Problem 15.3CYU: A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent...

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A student ran the following reaction in the laboratory at 744 K:

N₂(g) + 3H₂(g) 2NH₃(g)

When she introduced 4.00×10^-2 moles of N₂(g) and 5.96×10^-2 moles of H₂(g) into a 1.00 liter container, she found the equilibrium concentration of NH₃(g) to be 8.88×10^-4 M.

Calculate the equilibrium constant, K_c, she obtained for this reaction.

A student ran the following reaction in the laboratory at 744 K:
N2(g) + 3H2(g)
2NH3(g)
When she introduced 4.00x10-2 moles of N2(g) and 5.96×10 2 moles of H2(9) into
a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be
8.88x10-4 M.
Calculate the equilibrium constant, Ke, she obtained for this reaction.

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