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- 1. Multiple Choice
Electrons always flow from
cathode to anode
anode to cathode
- 2. Multiple Choice
Oxidation occurs at the
anode
cathode
- 3. Multiple Choice
Electrons are gained at the
anode
cathode
- 4. Multiple Choice
Given their standard reduction potentials, which of the species is going to be oxidized?
Cu2+/Cu = 0.34V
Zn2+/Zn = -0.76V
Cu
Zn
CuSO4
ZnSO4
- 5. Multiple Choice
An iron nail is put into a solution of copper nitrate, copper has a more positive reduction potential than iron, what will happen?
iron will be reduced
bubbles of oxygen gas will form on iron nail
the iron nail will become copper plated
no reaction occurs
- 6. Multiple Choice
What occurs to the mass of copper electrode in the following reaction?
Zn/Zn2+ // Cu2+/Cu
increases
decreases
remains the same
- 7. Multiple Choice
Which metal is the negative electrode?
Zn/Zn2+ // Cu2+/Cu
zinc
copper
- 8. Multiple Choice
What reaction occurs at the anode?
Ag+/Ag = 0.80V
Ni2+/Ni = -0.25V
Ag+ + e- →Ag
Ag → Ag+ + e-
Ni2+ + 2e- → Ni
Ni → Ni2+ + 2e-
- 9. Multiple Choice
What would be the theoretical cell potential of the previous electrochemical cell?
Ag+/Ag = 0.80V
Ni2+/Ni = -0.25V
1.05V
-1.05V
0.55V
-0.55V
- 10. Multiple Choice
Standard Conditions Galvanic Cells would be
1.0 M solutions
1 atm pressure
25o Celsius
all of the above
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