Suppose a 250. mL flask is filled with 1.7 mol of NO, 1.9 mol of CO and 0.40 mol of NO. The following reaction becomes possible: NO, (8) + CO(g) NO(g) + CO,(8) The equilibrium constant K for this reaction is 8.11 at the temperature of the flask. Calculate the equilibrium molarity of NO,. Round your answer to two decimal places. M ?.

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Chapter17: Equilibrium
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Suppose a 250. mL flask is filled with 1.7 mol of NO, 1.9 mol of CO and 0.40 mol of NO. The following reaction becomes possible:
NO, (8) + CO(g) NO(g) + CO,(8)
The equilibrium constant K for this reaction is 8.11 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 1.7 mol of NO, 1.9 mol of CO and 0.40 mol of NO. The following reaction becomes possible: NO, (8) + CO(g) NO(g) + CO,(8) The equilibrium constant K for this reaction is 8.11 at the temperature of the flask. Calculate the equilibrium molarity of NO,. Round your answer to two decimal places. M Explanation Check 2021 McGraw Hill Educati All Rights Reserved Terms of Use Privacy V 1 7:34 cer 8
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