Suppose a 500. mL flask is filled with 1.6 mol of H,0, 0.30 mol of CO, and 0.80 mol of H,. The following reaction becomes possible: Co(g) +H,O(g) – CO, (g) +H, (g) The equilibrium constant K for this reaction is 0.616 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. I| M
Suppose a 500. mL flask is filled with 1.6 mol of H,0, 0.30 mol of CO, and 0.80 mol of H,. The following reaction becomes possible: Co(g) +H,O(g) – CO, (g) +H, (g) The equilibrium constant K for this reaction is 0.616 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. I| M
General Chemistry - Standalone book (MindTap Course List)
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Chapter14: Chemical Equilibirum
Section: Chapter Questions
Problem 14.19QP: During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction...
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![Suppose a 500. mL flask is filled with 1.6 mol of H,O, 0.30 mol of CO, and 0.80 mol of H,. The following reaction becomes possible:
(3)7
CO( ) + H,O(g) = CO,() + H, (g)
The equilibrium constant K for this reaction is 0.616 at the temperature of the flask.
Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
) M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9ac4fab7-4126-49f3-8d16-60074d8271b3%2F95e56023-0bb6-4b78-b8d8-08b1b6846828%2Fgs7097s_processed.png&w=3840&q=75)
Transcribed Image Text:Suppose a 500. mL flask is filled with 1.6 mol of H,O, 0.30 mol of CO, and 0.80 mol of H,. The following reaction becomes possible:
(3)7
CO( ) + H,O(g) = CO,() + H, (g)
The equilibrium constant K for this reaction is 0.616 at the temperature of the flask.
Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
) M
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