
Nernst Equation and Cell Potential
Interactive Video
•
Chemistry, Physics, Science
•
11th - 12th Grade
•
Practice Problem
•
Hard
Patricia Brown
FREE Resource
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10 questions
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1.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
What happens to tin in the oxidation-reduction process described?
It remains unchanged.
It loses two electrons.
It gains two electrons.
It gains one electron.
2.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
In the standard electrode potential table, how are reactions typically written?
As reduction reactions.
As spontaneous reactions.
As neutral reactions.
As oxidation reactions.
3.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
Which electrode is always on the left in the cell notation?
Neither
Anode
Cathode
Both
4.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
How is the standard EMF of a cell calculated?
By adding the potentials of the anode and cathode.
By subtracting the anode potential from the cathode potential.
By multiplying the potentials of the anode and cathode.
By dividing the cathode potential by the anode potential.
5.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
What is the standard EMF of the cell if all concentrations are 1.0 molar?
0.001 volts
1.0 volts
0.01 volts
0.1 volts
6.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
What does the Nernst equation help calculate?
The standard EMF of a cell.
The cell potential under non-standard conditions.
The concentration of reactants.
The equilibrium constant.
7.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
What is the correction factor in the Nernst equation?
0.0592 divided by the number of electrons exchanged.
0.0592 multiplied by the number of electrons exchanged.
0.0592 added to the number of electrons exchanged.
0.0592 subtracted from the number of electrons exchanged.
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