Consider the reaction N₂(g) + O₂(g) 2 NO(g) that has an equilibrium constant, Ke, fof 4.10 x 10-4 at 1700 °C. What percentage of O₂ will react to form NO if 0.603 mol N₂ and 0.603 mol O₂ are added to a 0.901 L container and allowed to come to equilbrium at 1700 °C? percentage of 0₂: 1.41 %

Consider the reaction N₂(g) + O₂(g) 2 NO(g) that has an equilibrium constant, Ke, fof 4.10 x 10-4 at 1700 °C. What percentage of O₂ will react to form NO if 0.603 mol N₂ and 0.603 mol O₂ are added to a 0.901 L container and allowed to come to equilbrium at 1700 °C? percentage of 0₂: 1.41 %

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 15Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...

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Question

Consider the reaction
N₂(g) + O₂(g)
2 NO(g)
that has an equilibrium constant, Kc, fof 4.10 × 10-4 at 1700 °C. What percentage of O₂ will react to form NO if 0.603 mol N₂
and 0.603 mol O₂ are added to a 0.901 L. container and allowed to come to equilbrium at 1700 °C?
percentage of 0₂:
1.41
%

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Step 2: Calculate the concentration of reactants by the ratio between the mass of compound to the volume.

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Step 3: Calculate the concentration of product formed during the reaction using ICE

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Step 4: Find the value of x (the change in concentration)

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Step 5: Calculate the equilibrium concentration of O2

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