Suppose a 250. mL flask is filled with 1.0 mol of NO₂, 0.20 mol of NO and 1.7 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 5.54 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M X 5
Suppose a 250. mL flask is filled with 1.0 mol of NO₂, 0.20 mol of NO and 1.7 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 5.54 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M X 5
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 250. mL flask is filled with 1.0 mol of NO₂, 0.20 mol of NO and 1.7 mol of CO₂. The following reaction becomes possible:
NO₂(g) +CO(g) NO(g) +CO, (g)
The equilibrium constant K for this reaction is 5.54 at the temperature of the flask.
Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
M
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Transcribed Image Text:Suppose a 250. mL flask is filled with 1.0 mol of NO₂, 0.20 mol of NO and 1.7 mol of CO₂. The following reaction becomes possible:
NO₂(g) +CO(g) NO(g) +CO, (g)
The equilibrium constant K for this reaction is 5.54 at the temperature of the flask.
Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
M
Images
X
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