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Suppose a 500. mL flask is filled with 0.50 mol of CO, 0.70 mol of NO and 1.0 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.600 at the temperature of the flask. Calculate the equilibrium molarity of NO₂. Round your answer to two decimal places. M X

Suppose a 500. mL flask is filled with 0.50 mol of CO, 0.70 mol of NO and 1.0 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.600 at the temperature of the flask. Calculate the equilibrium molarity of NO₂. Round your answer to two decimal places. M X

World of Chemistry, 3rd edition
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 17A
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Suppose a 500. mL flask is filled with 0.50 mol of CO, 0.70 mol of NO and 1.0 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.600 at the temperature of the flask. Calculate the equilibrium molarity of NO₂. Round your answer to two decimal places. M X
Transcribed Image Text:Suppose a 500. mL flask is filled with 0.50 mol of CO, 0.70 mol of NO and 1.0 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.600 at the temperature of the flask. Calculate the equilibrium molarity of NO₂. Round your answer to two decimal places. M X
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