Consider the equilibrium H2(g) + Br2(g) ⇌ 2HBr(g) To a 20.0 L flask are added 0.100 moles of H2 and 0.200 moles of HBr. The equilibrium constant for this reaction is 989. Calculate the number of moles of Br2 in the flask when equilibrium is established. Make any reasonable approximation, clearly stating what that approximation is.
Consider the equilibrium H2(g) + Br2(g) ⇌ 2HBr(g) To a 20.0 L flask are added 0.100 moles of H2 and 0.200 moles of HBr. The equilibrium constant for this reaction is 989. Calculate the number of moles of Br2 in the flask when equilibrium is established. Make any reasonable approximation, clearly stating what that approximation is.
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 61QRT
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Consider the equilibrium
H2(g) + Br2(g) ⇌ 2HBr(g)
To a 20.0 L flask are added 0.100 moles of H2 and 0.200 moles of HBr. The equilibrium constant for this reaction is
989. Calculate the number of moles of Br2 in the flask when equilibrium is established. Make any reasonable
approximation, clearly stating what that approximation is.
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