Name: 
 

Chemistry 12 - Chapter 10 Quiz



True/False
Indicate whether the sentence or statement is true or false.
 

1. 

Electrolytic cells are based on nonspontaneous reactions and have a negative cell potential.
 

2. 

Reduction occurs at the anode and oxidation occurs at the cathode in an electrolytic cell.
 

3. 

Electrolytic cells generally have a single electrolyte so they are really half-cells with the power supply serving as the other half-cell.
 

4. 

The minimum potential difference for an aqueous cadmium sulfate cell with inert electrodes is 1.63 V.
 

5. 

The charge transferred in a cell is directly proportional to both the current and the time.
 

6. 

The mass of a nonmetal formed at the anode in an electrolytic cell is directly related to the amount of electrons transferred at the electrode.
 

7. 

If you want to deposit twice a given mass of silver in an electrolytic cell, then you must use twice the current for double the time.
 

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

8. 

In an electrolytic cell, electrons are transferred through the
a.
solution from the anode to the cathode.
b.
solution from the cathode to the anode.
c.
porous barrier from the cathode to the anode.
d.
external wire from the cathode to the anode.
e.
external wire from the anode to the cathode.
 

9. 

Oxidation and reduction half-reactions occur
a.
at the surface of an electrode.
b.
in the power supply.
c.
in the salt bridge.
d.
where the wire connects to the electrode.
e.
at the porous barrier.
 

10. 

In an electrolytic cell, the strongest oxidizing agent reacts at the
a.
anode and undergoes an oxidation.
b.
cathode and undergoes a reduction.
c.
anode and gains electrons.
d.
cathode and loses electrons.
e.
porous barrier and transfers electrons.
 

11. 

If we assume standard conditions, what is the cell potential for the cell
Pt(s) | ZnBr2(aq) | Pt(s)?
a.
+1.83 V
b.
+0.31 V
c.
-0.07 V
d.
-1.83V
e.
-2.06V
 

12. 

What are the products obtained at the electrodes in the following cell with a small potential difference applied?
Sn(s) | Sn(NO3)2(aq) | Sn(s)
 
cathode
anode
a
Sn2+(aq)
Sn4+(aq)
b
Sn(s)
Sn2+(aq)
c
H2(g), OH-(aq)
O2(g), H+(aq)
d
NO2(g), H2O(l)
Sn2+(aq)
e
Sn4+(aq)
Sn2+(aq)
a.
a
b.
b
c.
c
d.
d
e.
e
 

13. 

The Faraday constant relates
a.
charge and current.
b.
current and time.
c.
time and mass.
d.
mass and charge of electrons.
e.
charge and amount of electrons.
 

14. 

In the electrolysis of aqueous potassium hydroxide with inert electrodes, the product(s) at the anode will be
a.
O2(g), H+(aq)
b.
K(s)
c.
O2(g), H2O(l)
d.
H2(g), OH-(aq)
e.
KOH(s)
 

15. 

The mass of the gas produced at the anode in the electrolysis of aqueous potassium hydroxide using 5.9 A of current for 22 min is
a.
0.65 g.
b.
0.32 g.
c.
0.081 g.
d.
0.020 g.
e.
0.017 g
 

16. 

Electrolytic cells used in industrial processes may do all of the following except
a.
produce elements.
b.
refine metals.
c.
plate metals.
d.
produce electricity.
e.
act as cathodic protectors.
 



 
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