Determine the oxidation number of the chromium in an undetermined salt solution if electrolysis of a molten sample of this salt for 1.50 hours with a 10.0 A current deposit 9.71 grams of chromium metal at the cathode (use 52g/mol as molar mass of Chromium; Faraday constant = 96485 C/mol e.). Hints: (1) Get the number of moles of electrons. Note that ampere means coulombs per second (C/s). (2) Get the number of moles of Chromium deposited. (3) Get the ratio of mol e and mole Cr.
Determine the oxidation number of the chromium in an undetermined salt solution if electrolysis of a molten sample of this salt for 1.50 hours with a 10.0 A current deposit 9.71 grams of chromium metal at the cathode (use 52g/mol as molar mass of Chromium; Faraday constant = 96485 C/mol e.). Hints: (1) Get the number of moles of electrons. Note that ampere means coulombs per second (C/s). (2) Get the number of moles of Chromium deposited. (3) Get the ratio of mol e and mole Cr.
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 102CP
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Transcribed Image Text:Determine the oxidation number of the chromium in an undetermined salt solution if electrolysis of a
molten sample of this salt for 1.50 hours with a 10.0 A current deposit 9.71 grams of chromium metal at
the cathode (use 52g/mol as molar mass of Chromium; Faraday constant = 96485 C/mol e.).
Hints:
(1) Get the number of moles of electrons. Note that ampere means coulombs per second (C/s).
(2) Get the number of moles of Chromium deposited.
(3) Get the ratio of mol e and mole Cr.
Oxidation number in this case refers to the charge of the ion. Input the value of the oxidation number (no symbols included).
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