When 0.02 moles of NOBr are added to a 2.00 L flask at 300 degrees C and the decomposition reaction 2NOBr(g) ⇄ 2NO(g) + Br2(g) comes to equilibrium, the partial pressure of the NOBr is 0.17 Atm. What is the equilibrium constant Kp?
When 0.02 moles of NOBr are added to a 2.00 L flask at 300 degrees C and the decomposition reaction 2NOBr(g) ⇄ 2NO(g) + Br2(g) comes to equilibrium, the partial pressure of the NOBr is 0.17 Atm. What is the equilibrium constant Kp?
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 110QRT:
The diagram represents an equilibrium mixture for the reaction
N2(g) + O2(g) ⇌ 2 NO(g)
Estimate the...
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When 0.02 moles of NOBr are added to a 2.00 L flask at 300 degrees C and the decomposition reaction 2NOBr(g) ⇄ 2NO(g) + Br2(g) comes to equilibrium, the partial pressure of the NOBr is 0.17 Atm. What is the equilibrium constant Kp?
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