Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g) + O2 (g) → 2 NO (g) The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.300 mol N2 and 0.980 mol O2 are mixed in a 5.00-L reaction vessel. What will be the concentrations of N2, O2, and NO when equilibrium is established?
Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g) + O2 (g) → 2 NO (g) The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.300 mol N2 and 0.980 mol O2 are mixed in a 5.00-L reaction vessel. What will be the concentrations of N2, O2, and NO when equilibrium is established?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 41QRT: Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures.
2 NOCl(g) ⇌ 2 NO(g) +...
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Nitrogen and oxygen react to produce nitric oxide according to the following equation:
N2 (g) + O2 (g) → 2 NO (g)
The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.300 mol N2 and 0.980 mol O2 are mixed in a 5.00-L reaction vessel. What will be the concentrations of N2, O2, and NO when equilibrium is established? (Hint: assume that the amounts of N2 and O2 that react are small—less than 10% of the starting amounts—and check your assumption when you have solved the equation.)
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