3. Consider the following galvanic cell: Fe(s) Cr(s) Salt bridge- containing KNO,(aq) IM Fe+ IM Cr+ a. Write the half reaction that occurs at the cathode. b. Write the half reaction that occurs at the anode. c. Calculate the Ecell. d. Write the overall redox reaction. e. What happens to the mass of the Fe electrode as the redox reaction progresses? f. What happens the concentration of The Fe3+ ion as the reaction progresses? g. Which chamber will the nitrate ion flow into? (anode or cathode)
3. Consider the following galvanic cell: Fe(s) Cr(s) Salt bridge- containing KNO,(aq) IM Fe+ IM Cr+ a. Write the half reaction that occurs at the cathode. b. Write the half reaction that occurs at the anode. c. Calculate the Ecell. d. Write the overall redox reaction. e. What happens to the mass of the Fe electrode as the redox reaction progresses? f. What happens the concentration of The Fe3+ ion as the reaction progresses? g. Which chamber will the nitrate ion flow into? (anode or cathode)
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 105QAP: Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a)...
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