1. Calculate the equilibrium concentration value (K) forhomogeneous reaction:2Fe³+ + 21 = 1₂ ) + 2Fe²+ 90% of Fe³+ ions have reacted by2 (1)(1)*the equilibrium moment. Initial concentrations are: Co (Fe³+) =1∙10-³ (mol/L), C (I) = 1·10˚³ (mol/L).0

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1. Calculate the equilibrium concentration value (K) for homogeneous reaction: 2Fe³+ + 21 (1) = = 1₂ +2Fe²+. 90% of Fe³+ ions have reacted by (1) 2 (1) the equilibrium moment. Initial concentrations are: Co (Fe³+): 1-10-³ (mol/L), C, (I) = 1.10³ (mol/L). =

1. Calculate the equilibrium concentration value (K) for homogeneous reaction: 2Fe³+ + 21 (1) = = 1₂ +2Fe²+. 90% of Fe³+ ions have reacted by (1) 2 (1) the equilibrium moment. Initial concentrations are: Co (Fe³+): 1-10-³ (mol/L), C, (I) = 1.10³ (mol/L). =

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 37P

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Question

1. Calculate the equilibrium concentration value (K) for
homogeneous reaction:
2Fe³+ + 21 = 1₂ ) + 2Fe²+ 90% of Fe³+ ions have reacted by
2 (1)
(1)*
the equilibrium moment. Initial concentrations are: Co (Fe³+) =
1∙10-³ (mol/L), C (I) = 1·10˚³ (mol/L).
0

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