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A student ran the following reaction in the laboratory at 709 K: N2(g) + 3H2(g)2NH3(g) When she introduced 4.04x102 moles of N(g) and 6.09x102 moles of H2ig) into a 1.00 liter container, she found the equilibrium concentration of H2lg) to be 5.89x102 M. Calculate the equilibrium constant, K. she obtained for this reaction.

A student ran the following reaction in the laboratory at 709 K: N2(g) + 3H2(g)2NH3(g) When she introduced 4.04x102 moles of N(g) and 6.09x102 moles of H2ig) into a 1.00 liter container, she found the equilibrium concentration of H2lg) to be 5.89x102 M. Calculate the equilibrium constant, K. she obtained for this reaction.

Chemistry & Chemical Reactivity
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
Section15.4: Using Equilibrium Constants In Calculations
Problem 15.5CYU: The decomposition of PCl5(g) to form PCl3(g) and Cl2(g) has Kc = 33.3 at a high temperature. If the...
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A student ran the following reaction in the laboratory at 709 K: N2g) + 3H2(g)2NH3(g) When she introduced 4.04x102 moles of N(g) and 6.09x102 moles of H2ig) into a 1.00 liter container, she found the equilibrium concentration of H2lg) to be 5.89x102 M. Calculate the equilibrium constant, K. she obtained for this reaction. K =
Transcribed Image Text:A student ran the following reaction in the laboratory at 709 K: N2g) + 3H2(g)2NH3(g) When she introduced 4.04x102 moles of N(g) and 6.09x102 moles of H2ig) into a 1.00 liter container, she found the equilibrium concentration of H2lg) to be 5.89x102 M. Calculate the equilibrium constant, K. she obtained for this reaction. K =
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