2.50 mol NOCl was placed in a 2.50 L reaction vessel at 400ºC. After equilibrium was established, it was found that 28.0% of the NOCl had dissociated according to the equation 2NOCl(g) <--> 2NO(g) + Cl2(g). Calculate the equilibrium constant, Kc, for the reaction. (3 sig figs) ( ICE table with all numbers, no unknown x)
2.50 mol NOCl was placed in a 2.50 L reaction vessel at 400ºC. After equilibrium was established, it was found that 28.0% of the NOCl had dissociated according to the equation 2NOCl(g) <--> 2NO(g) + Cl2(g). Calculate the equilibrium constant, Kc, for the reaction. (3 sig figs) ( ICE table with all numbers, no unknown x)
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 9QRT
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2.50 mol NOCl was placed in a 2.50 L reaction vessel at 400ºC. After equilibrium was established, it was found that 28.0% of the NOCl had dissociated according to the equation 2NOCl(g) <--> 2NO(g) + Cl2(g).
Calculate the equilibrium constant, Kc, for the reaction. (3 sig figs)
( ICE table with all numbers, no unknown x)
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