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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 × 10¬ª at a high temperature. If 0.20 mol N2 and 0.15 mol O2 react in a 1.0 L vessel, what will the equilibrium concentration of O2 be?

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 × 10¬ª at a high temperature. If 0.20 mol N2 and 0.15 mol O2 react in a 1.0 L vessel, what will the equilibrium concentration of O2 be?

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter13: Fundamental Equilibrium Concepts
Section: Chapter Questions
Problem 12E: Show that the complete chemical equation, the total ionic equation, and the net ionic equation for...
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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 x 10-4 at a high temperature. If 0.20 mol N2 and 0.15 mol O2 react in a 1.0 L vessel, what will the equilibrium concentration of O2 be? N2(g) + O2(g) =2 NO(g) 1 2 3 4 NEXT > Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms. Qc %3D II
Transcribed Image Text:Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 x 10-4 at a high temperature. If 0.20 mol N2 and 0.15 mol O2 react in a 1.0 L vessel, what will the equilibrium concentration of O2 be? N2(g) + O2(g) =2 NO(g) 1 2 3 4 NEXT > Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms. Qc %3D II
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