Suppose a 250. mL flask is filled with 0.30 mol of NO and 0.80 mol of NO2. The following reaction becomes possible: NO3(g)+NO(g)<->2NO2(g) The equilibrium constant K for this reaction is 0.717 at the temperature of the flask. Calculate the equilibrium molarity of NO2. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 0.30 mol of NO and 0.80 mol of NO2. The following reaction becomes possible: NO3(g)+NO(g)<->2NO2(g) The equilibrium constant K for this reaction is 0.717 at the temperature of the flask. Calculate the equilibrium molarity of NO2. Round your answer to two decimal places.
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
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 3ALQ: For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each...
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Suppose a 250. mL flask is filled with 0.30 mol of NO and 0.80 mol of NO2. The following reaction becomes possible:
NO3(g)+NO(g)<->2NO2(g)
The equilibrium constant K for this reaction is 0.717 at the temperature of the flask.
Calculate the equilibrium molarity of NO2. Round your answer to two decimal places.
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