The equilibrium constant for the dissociation of moleculariodine, I2(g)⇌ 2 I(g), at 800 K is Kc = 3.1 x10-5.(a) Which species predominates at equilibrium I2 or I?(b) Assuming both forward and reverse reactions areelementary processes, which reaction has the larger rateconstant, the forward or the reverse reaction?
The equilibrium constant for the dissociation of moleculariodine, I2(g)⇌ 2 I(g), at 800 K is Kc = 3.1 x10-5.(a) Which species predominates at equilibrium I2 or I?(b) Assuming both forward and reverse reactions areelementary processes, which reaction has the larger rateconstant, the forward or the reverse reaction?
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 56QRT
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The equilibrium constant for the dissociation of molecular
iodine, I2(g)⇌ 2 I(g), at 800 K is Kc = 3.1 x10-5.
(a) Which species predominates at equilibrium I2 or I?
(b) Assuming both forward and reverse reactions are
elementary processes, which reaction has the larger rate
constant, the forward or the reverse reaction?
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