N2 (1.25 mol) and O, (0.75 mol) were placed in a one liter flask and allowed to reach equilibrium at 500 K according to the equation below. At equilibrium, the flask contains 1.00 mol of NO. Calculate the equilibrium-constant K. for this reaction. N2 (g) + 0, (g) 2 NO (g).

Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.40QE
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N2 (1.25 mol) and O, (0.75 mol) were placed in a one liter flask and allowed
to reach equilibrium at 500 K according to the equation below. At equilibrium, the flask
contains 1.00 mol of NO. Calculate the equilibrium-constant K, for this reaction.
N2 (g) + 0, (g)
2 NO (g).
Transcribed Image Text:N2 (1.25 mol) and O, (0.75 mol) were placed in a one liter flask and allowed to reach equilibrium at 500 K according to the equation below. At equilibrium, the flask contains 1.00 mol of NO. Calculate the equilibrium-constant K, for this reaction. N2 (g) + 0, (g) 2 NO (g).
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