Suppose a 250. mL flask is filled with 0.20 mol of NO₂, 0.50 mol of NO and 0.40 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) → NO(g) + CO₂(g) The equilibrium constant K for this reaction is 6.83 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 0.20 mol of NO₂, 0.50 mol of NO and 0.40 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) → NO(g) + CO₂(g) The equilibrium constant K for this reaction is 6.83 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 51QRT: At room temperature, the equilibrium constant Kc for the reaction
2 NO(g) ⇌ N2(g) + O2(g)
is 1.4 ×...
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