A student measures the potential of a cell made up with 1.0 M CuSO4 in one solution and 1.0 M AgNO3 in the other. There is a Cu electrode in the CuSO4 solution and an Ag electrode in the AgNO3 solution. The salt bridge connects the two half-cells. The student finds that the potential, or voltage of the cell is 0.46 V and that the Cu electrode is negative. a) At which electrode is the oxidation occurring? ______________________________________ b) Write the balanced equation for the oxidation reaction. ________________________________ c) Write the balanced equation for the reduction reaction. ________________________________ d) Write the balanced redox reaction.
A student measures the potential of a cell made up with 1.0 M CuSO4 in one solution and 1.0 M AgNO3 in the other. There is a Cu electrode in the CuSO4 solution and an Ag electrode in the AgNO3 solution. The salt bridge connects the two half-cells. The student finds that the potential, or voltage of the cell is 0.46 V and that the Cu electrode is negative. a) At which electrode is the oxidation occurring? ______________________________________ b) Write the balanced equation for the oxidation reaction. ________________________________ c) Write the balanced equation for the reduction reaction. ________________________________ d) Write the balanced redox reaction.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 97QRT
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A student measures the potential of a cell made up with 1.0 M CuSO4 in one solution and 1.0 M AgNO3 in the other. There is a Cu electrode in the CuSO4 solution and an Ag electrode in the AgNO3 solution. The salt bridge connects the two half-cells. The student finds that the potential, or voltage of the cell is 0.46 V and that the Cu electrode is negative.
- a) At which electrode is the oxidation occurring? ______________________________________
- b) Write the balanced equation for the oxidation reaction. ________________________________
- c) Write the balanced equation for the reduction reaction. ________________________________
- d) Write the
balanced redox reaction. _______________________________________________
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