5. Consider the following under acidic conditions: Cu(s) + MnO4¹ (aq) → Mn²+ + Cu²+iiiWrite the balanced half-reactionfor the oxidation that occurs.Write the balanced half-reactionfor the reduction that occurs.iii Write the balanced redox reaction.iv Write the potential for each half-reaction next to it (the values are in your text)V Calculate the cell potential.vi Calculate AG at 25 °C.vii Is this reaction spontaneous? Why?viii Draw and label the cell for this reaction.ix Write the line notation for the cell.

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5. Consider the following under acidic conditions: Cu(s) + MnO4¹(aq) → Mn²+ + Cu²+ Write the balanced half-reaction for the oxidation that occurs. i ii Write the balanced half-reaction for the reduction that occurs. iii Write the balanced redox reaction.

5. Consider the following under acidic conditions: Cu(s) + MnO4¹(aq) → Mn²+ + Cu²+ Write the balanced half-reaction for the oxidation that occurs. i ii Write the balanced half-reaction for the reduction that occurs. iii Write the balanced redox reaction.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

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5. Consider the following under acidic conditions: Cu(s) + MnO4¹ (aq) → Mn²+ + Cu²+
i
ii
Write the balanced half-reaction
for the oxidation that occurs.
Write the balanced half-reaction
for the reduction that occurs.
iii Write the balanced redox reaction.
iv Write the potential for each half-reaction next to it (the values are in your text)
V Calculate the cell potential.
vi Calculate AG at 25 °C.
vii Is this reaction spontaneous? Why?
viii Draw and label the cell for this reaction.
ix Write the line notation for the cell.

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