Suppose a 500. mL flask is filled with 1.9 mol of NO3 and 0.50 mol of NO,. The following reaction becomes possible: NO,(2) + NO(2) → 2NO,(3) The equilibrium constant K for this reaction is 4.80 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. ?
Suppose a 500. mL flask is filled with 1.9 mol of NO3 and 0.50 mol of NO,. The following reaction becomes possible: NO,(2) + NO(2) → 2NO,(3) The equilibrium constant K for this reaction is 4.80 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. ?
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 17A
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Question
![Suppose a 500. mL flask is filled with 1.9 mol of NO, and 0.50 mol of NO,. The following reaction becomes possible:
NO, (2) +NO(g) – 2NO, (g)
The equilibrium constant K for this reaction is 4.80 at the temperature of the flask.
Calculate the equilibrium molarity of NO3. Round your answer to two decimal places.
M
?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F20cb9ae6-0091-4933-a633-5de5cc0a2b63%2F49f4119d-e566-4490-a790-317b5463417d%2Fl1h49ab_processed.png&w=3840&q=75)
Transcribed Image Text:Suppose a 500. mL flask is filled with 1.9 mol of NO, and 0.50 mol of NO,. The following reaction becomes possible:
NO, (2) +NO(g) – 2NO, (g)
The equilibrium constant K for this reaction is 4.80 at the temperature of the flask.
Calculate the equilibrium molarity of NO3. Round your answer to two decimal places.
M
?
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