A sample of an iron containing ore is crushed and powder is extracted to form a clear aqueous solution. A clean iron electrode is immersed into the solution and the cell shown below is made + Fe|Fe2+ (aq) | | SCE The e.m.f at equilibrium is 0.714 V at 298 K. (Esec = 0.242V, E° Fe2+|Fe = -0.44V) Calculate the concentration of Fe 2+ in the sample.
A sample of an iron containing ore is crushed and powder is extracted to form a clear aqueous solution. A clean iron electrode is immersed into the solution and the cell shown below is made + Fe|Fe2+ (aq) | | SCE The e.m.f at equilibrium is 0.714 V at 298 K. (Esec = 0.242V, E° Fe2+|Fe = -0.44V) Calculate the concentration of Fe 2+ in the sample.
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
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 77AP
Related questions
Question
A sample of an iron containing ore is crushed and powder is extracted to form a clear
aqueous solution. A clean iron electrode is immersed into the solution and the cell shown
below is made
+
Fe|Fe2+ (aq) | | SCE
The e.m.f at equilibrium is 0.714 V at 298 K. (Esec = 0.242V, E° Fe2+|Fe = -0.44V)
Calculate the concentration of Fe 2+ in the sample.
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