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NO and O2 (g) are mixed in a container of fixed volume and kept at 1000 K. Their initial concentrations are 0.0200 mol/L and 0.0300 mol/ L, respectively. When the reaction, NO(g) + O2 (g) = NO₂ has come to equilibrium, the concentration of NO2 (g) is 2.1 x 103 mol/L. Calculate the equilibrium constant, K, for the reaction. 0.2857 2.1035 3.5000 O 0.4754

NO and O2 (g) are mixed in a container of fixed volume and kept at 1000 K. Their initial concentrations are 0.0200 mol/L and 0.0300 mol/ L, respectively. When the reaction, NO(g) + O2 (g) = NO₂ has come to equilibrium, the concentration of NO2 (g) is 2.1 x 103 mol/L. Calculate the equilibrium constant, K, for the reaction. 0.2857 2.1035 3.5000 O 0.4754

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
Section15.3: 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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NO and O2 (g) are mixed in a container of fixed volume and kept at 1000 K. Their initial concentrations are 0.0200 mol/L and 0.0300 mol/L, respectively. When the reaction, NO (g) + O2 (g) = NO2 (g) has come to equilibrium, the concentration of NO2 (g) is 2.1 x 10-3 mol/L. Calculate the equilibrium constant, K, for the reaction. 0.2857 2.1035 3.5000 0.4754 O
Transcribed Image Text:NO and O2 (g) are mixed in a container of fixed volume and kept at 1000 K. Their initial concentrations are 0.0200 mol/L and 0.0300 mol/L, respectively. When the reaction, NO (g) + O2 (g) = NO2 (g) has come to equilibrium, the concentration of NO2 (g) is 2.1 x 10-3 mol/L. Calculate the equilibrium constant, K, for the reaction. 0.2857 2.1035 3.5000 0.4754 O
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