5. If 2.46 g of Fe 2+ were oxidized in the reaction Fe2+(aq) + Ce4+( aq ) à Fe3+ (aq) + Ce3+ (aq ), how many coulombs of charge must have been transferred from V2+ to Fe3+ ? Given Faraday constant F = 96490 C/mol e- , A.W.Fe = 55.85 g/mol. how many seconds must have been passed if a constant electric current 1.5 amperes were maintained?
5. If 2.46 g of Fe 2+ were oxidized in the reaction Fe2+(aq) + Ce4+( aq ) à Fe3+ (aq) + Ce3+ (aq ), how many coulombs of charge must have been transferred from V2+ to Fe3+ ? Given Faraday constant F = 96490 C/mol e- , A.W.Fe = 55.85 g/mol. how many seconds must have been passed if a constant electric current 1.5 amperes were maintained?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter20: Chemistry Of Selected Transition Elements And Coordination Compounds
Section20.5: Chromium
Problem 20.5PSP: At what pH does Ecell = 0.00 V for the reduction of dichromate by iodide ion in acid solution,...
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5. If 2.46 g of Fe 2+ were oxidized in the reaction Fe2+(aq) + Ce4+( aq ) à Fe3+ (aq) + Ce3+ (aq ),
- how many coulombs of charge must have been transferred from V2+ to Fe3+ ? Given Faraday constant F = 96490 C/mol e- , A.W.Fe = 55.85 g/mol.
- how many seconds must have been passed if a constant
electric current 1.5 amperes were maintained?
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