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Suppose a 500 ml flask is filled with 0.90 mol of NO₂, 0.40 mol of CO and 1.3 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) + CO₂(g) The equilibrium constant & for this reaction is 0.990 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M

Suppose a 500 ml flask is filled with 0.90 mol of NO₂, 0.40 mol of CO and 1.3 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) + CO₂(g) The equilibrium constant & for this reaction is 0.990 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.52QE: Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium...
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X 17 X 18 M X 19 20 X 21 22 23 24 25 Suppose a 500. mL flask is filled with 0.90 mol of NO₂, 0.40 mol of CO and 1.3 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.990 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. 26 27 28 29 ? 圖 8 民□□图] E Ar M
Transcribed Image Text:X 17 X 18 M X 19 20 X 21 22 23 24 25 Suppose a 500. mL flask is filled with 0.90 mol of NO₂, 0.40 mol of CO and 1.3 mol of CO₂. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.990 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. 26 27 28 29 ? 圖 8 民□□图] E Ar M
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