1. Answer the following questions: a) Why aqueous solutions of KMN04 are not entirely stable? b) What factors affect the decomposition of KMNO4? c) How can you prepare 1L of 0.01M solution of KMnO4 (FW = 158.04g) in the laboratory? 2. Derive and Calculate the equilibrium constant of the reaction? 2 Fe3+ + 31 --→ 2 Fe2+ + I3- 2 Fe3+ + 2 e + 2 e 2 Fe+ 31 E= 0.771 V E = 0.536 V
1. Answer the following questions: a) Why aqueous solutions of KMN04 are not entirely stable? b) What factors affect the decomposition of KMNO4? c) How can you prepare 1L of 0.01M solution of KMnO4 (FW = 158.04g) in the laboratory? 2. Derive and Calculate the equilibrium constant of the reaction? 2 Fe3+ + 31 --→ 2 Fe2+ + I3- 2 Fe3+ + 2 e + 2 e 2 Fe+ 31 E= 0.771 V E = 0.536 V
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 23QAP: Ammonium carbamate solid (NH4CO2NH2) decomposes at 313 K into ammonia and carbon dioxide gases. At...
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