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1. Consider a cell buffered at pH 2.00 and consists of Fe2+(aq) (0.004 M), Fe3+(aq) (0.070 M) and MnO4-(aq) (0.024M), Mn2+(aq) (0.050 M), in which Fe2+ reduces MnO4- to Mn2+. a. Write the balanced reaction. b. What is the standard cell potential? Is the cell galvanic or electrolytic? c. What is the actual cell potential at 35.0oC?

1. Consider a cell buffered at pH 2.00 and consists of Fe2+(aq) (0.004 M), Fe3+(aq) (0.070 M) and MnO4-(aq) (0.024M), Mn2+(aq) (0.050 M), in which Fe2+ reduces MnO4- to Mn2+. a. Write the balanced reaction. b. What is the standard cell potential? Is the cell galvanic or electrolytic? c. What is the actual cell potential at 35.0oC?

Principles of Modern Chemistry
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 43P
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1. Consider a cell buffered at pH 2.00 and consists of Fe2+(aq) (0.004 M), Fe3+(aq) (0.070 M) and MnO4-(aq) (0.024M), Mn2+(aq) (0.050 M), in which Fe2+ reduces MnO4- to Mn2+.
a. Write the balanced reaction.
b. What is the standard cell potential? Is the cell galvanic or electrolytic?
c. What is the actual cell potential at 35.0oC?

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