Zn2+(aq) + 2e → Zn (s) E°red = -O.76 V½ O2 (g)+ H2O + 2e¯ → 2 OH (aq) Eºred =+0.40 VUse the reduction potential above tosolve for the cell potential E°cell in voltsfor the corrosion of copper:Zn (s) + ½ O2 (g) + H2O → Zn²* (aq) +20H (aq) From the result above, the cell potentialfor the corrosion of Zinc is higher thaniron. The oxidation/corrosion of copperis a MORE spontaneous reactioncompared to the oxidation/corrosion ofiron. Therefore, zinc is more prone tooxidation compared to iron. We can saythat zinc is a more active metal thaniron.Using the result for Nail D:Does wrapping Zinc strip prevented theIron nail from undergoingoxidation/rusting/corrosion?

The cell reaction for corrosion of zinc is as below: Zn(s) + 1/2 O2 (g) + H2O (l) -------> Zn2+…

Answered: Use the reduction potential above to…

Use the reduction potential above to solve for the cell potential E°cell in volts for the corrosion of copper: Zn (s) + ½ O2 (g) + H2O → Zn²* (aq) + 20H (aq)

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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Concept explainers

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.

Question

Zn2+
(aq) + 2e → Zn (s) E°red = -O.76 V
½ O2 (g)+ H2O + 2e¯ → 2 OH (aq) Eºred =
+0.40 V
Use the reduction potential above to
solve for the cell potential E°cell in volts
for the corrosion of copper:
Zn (s) + ½ O2 (g) + H2O → Zn²* (aq) +
20H (aq)

From the result above, the cell potential
for the corrosion of Zinc is higher than
iron. The oxidation/corrosion of copper
is a MORE spontaneous reaction
compared to the oxidation/corrosion of
iron. Therefore, zinc is more prone to
oxidation compared to iron. We can say
that zinc is a more active metal than
iron.
Using the result for Nail D:
Does wrapping Zinc strip prevented the
Iron nail from undergoing
oxidation/rusting/corrosion?

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