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Suppose a 250. mL flask is filled with 1.6 mol of NO₂, 0.20 mol of CO and 2.0 mol of NO. The following reaction becomes possible: NO₂(g) + CO(g) → NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.773 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X 3

Suppose a 250. mL flask is filled with 1.6 mol of NO₂, 0.20 mol of CO and 2.0 mol of NO. The following reaction becomes possible: NO₂(g) + CO(g) → NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.773 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X 3

Living By Chemistry: First Edition Textbook
Living By Chemistry: First Edition Textbook
1st Edition
ISBN:9781559539418
Author:Angelica Stacy
Publisher:Angelica Stacy
ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium
SectionU6.4: How Favorable: Equilibrium Constank K
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Suppose a 250. mL flask is filled with 1.6 mol of NO₂, 0.20 mol of CO and 2.0 mol of NO. The following reaction becomes possible: NO₂(g) + CO(g) → NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.773 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X 3
Transcribed Image Text:Suppose a 250. mL flask is filled with 1.6 mol of NO₂, 0.20 mol of CO and 2.0 mol of NO. The following reaction becomes possible: NO₂(g) + CO(g) → NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.773 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X 3
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