Problem Page suppose a 500.mL flask is filled with 0.60mol of NO and 1.8mol of NO2 . The following reaction becomes possible: +NO3gNOg <-> 2NO2g The equilibrium constant K for this reaction is 0.645 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places.
Problem Page suppose a 500.mL flask is filled with 0.60mol of NO and 1.8mol of NO2 . The following reaction becomes possible: +NO3gNOg <-> 2NO2g The equilibrium constant K for this reaction is 0.645 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places.
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter17: Chemical Equilibrium
Section17.3: Using Equilibrium Constants
Problem 27SSC
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suppose a 500.mL flask is filled with 0.60mol of NO and 1.8mol of NO2
. The following reaction becomes possible:
+NO3gNOg <-> 2NO2g
The equilibrium constant K for this reaction is 0.645 at the temperature of the flask.
Calculate the equilibrium molarity of NO3. Round your answer to two decimal places.
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