Suppose a 250. mL flask is filled with 0.50 mol of CO, 0.10 mol of NO and 1.6 mol of CO2. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 7.24 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X
Suppose a 250. mL flask is filled with 0.50 mol of CO, 0.10 mol of NO and 1.6 mol of CO2. The following reaction becomes possible: NO₂(g) + CO(g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 7.24 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Suppose a
250.mL
flask is filled with
0.50mol
of
CO
,
0.10mol
of
NO
and
1.6mol
of
CO2
. The following reaction becomes possible:
+NO2gCOg
+NOgCO2g
The equilibrium constant
K
for this reaction is
7.24
at the temperature of the flask.
Calculate the equilibrium molarity of
CO
. Round your answer to two decimal places.
Transcribed Image Text:Suppose a 250. mL flask is filled with 0.50 mol of CO, 0.10 mol of NO and 1.6 mol of CO2. The following reaction becomes possible:
NO₂(g) + CO(g) NO(g) + CO₂(g)
The equilibrium constant K for this reaction is 7.24 at the temperature of the flask.
Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
M
X
Transcribed Image Text:Suppose a 250. mL flask is filled with 0.50 mol of CO, 0.10 mol of NO and 1.6 mol of CO2. The following reaction becomes possible:
NO₂(g) + CO(g) → NO(g) + CO₂(g)
The equilibrium constant K for this reaction is 7.24 at the temperature of the flask.
Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
M
X
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