# Suppose a 250.mL flask is filled with 0.80mol of CO, 0.60mol of NO and 0.20mol of CO2. The following reaction becomes possible:NO2(g)+CO(g) <->NO(g)+CO2(g)The equilibrium constant K for this reaction is 9.16 at the temperature of the flask.Calculate the equilibrium molarity of NO. Round your answer to two decimal places.please check your work. most people get this wrong!

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Suppose a 250.mL flask is filled with 0.80mol of CO, 0.60mol of NO and 0.20mol of CO2. The following reaction becomes possible:

NO2(g)+CO(g) <->NO(g)+CO2(g)

The equilibrium constant K for this reaction is 9.16 at the temperature of the flask.

Calculate the equilibrium molarity of NO. Round your answer to two decimal places.

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Step 1

The initial concentrations of CO, NO and CO2 are calculated as shown below.

250 mL = 0.250 L help_outlineImage TranscriptioncloseNo. of moles of solute Concentration Volume(mL 0.8 - 3.2M 0.25 Initial[CO 0.6 = 2.4M 0.25 Initi al [NO] 0.8 0.8M Initial[CO,1= 0.25 fullscreen
Step 2

Equilibrium molarity of NO3 can be determined: help_outlineImage TranscriptioncloseNO Со NO CO. + + Initial 0 3.2 2.4 0.8 Change +x +x X -X Equilibrium 3.2-x 2.4+x 0.8+x х fullscreen
Step 3

K can be give... help_outlineImage Transcriptionclose[(2.4+x)(0.8+x [(x)(3.2-x) K= [(2.4+x0.8) 9.16= x)(3.2-x x 2.49 or 0.07 [NO, 2.49 or 0.07 fullscreen

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### Equilibrium Concepts 