A chemist designs a galvanic cell that uses these two half-reactions:2 H₂O(1)+2e2+Zn² (aq) +2eWrite a balancedequation for thehalf-reaction thathappens at thecathode.Write a balancedequation for thehalf-reaction thathappens at theanode.Answer the following questions about this cell.Write a balancedequation for theoverall reactionthat powers thecell. Be sure thereaction isspontaneous aswritten.Do you haveenoughhalf-reactioninformation tocalculate the cellvoltage understandardconditions?significant digit00YesNoIf you said it waspossible tocalculate the cellvoltage, do so andenter your answer ☐Vhere. Round youranswer to 1H₂(g) + 2 OH (aq)Zn(s)standard reduction potentialEºredEve'red0.83 V==- 0.763 Vロ→ロX90x10

1]Oxidation Reaction:Oxidation is a chemical process in which a substance loses electrons.It is…

Answered: half-reaction 2 H₂O(1)+2e H₂(g) + 2 OH…

half-reaction 2 H₂O(1)+2e H₂(g) + 2 OH (aq) 2+ Zn (aq) +2e Zn(s) standard reduction potential Ed -0.83 V red 'red -0.763 V

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

A chemist designs a galvanic cell that uses these two half-reactions:
2 H₂O(1)+2e
2+
Zn² (aq) +2e
Write a balanced
equation for the
half-reaction that
happens at the
cathode.
Write a balanced
equation for the
half-reaction that
happens at the
anode.
Answer the following questions about this cell.
Write a balanced
equation for the
overall reaction
that powers the
cell. Be sure the
reaction is
spontaneous as
written.
Do you have
enough
half-reaction
information to
calculate the cell
voltage under
standard
conditions?
significant digit
0
0
Yes
No
If you said it was
possible to
calculate the cell
voltage, do so and
enter your answer ☐V
here. Round your
answer to 1
H₂(g) + 2 OH (aq)
Zn(s)
standard reduction potential
Eº
red
Eve
'red
0.83 V
==
- 0.763 V
ロ→ロ
X
90
x10

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Step 2: Balanced Half-cell that happens at cathode

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Step 3: Balanced Half-cell that happens at anode

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Step 4: Net balanced equation

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Step 5: Evaluate cell voltage under standard conditions

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