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Oxidation, reduction, electrochemical cells, electrolytic

Total questions: 46

Worksheet time: 44mins

Name
Class
Date
1.
Which cell is not spontaneous?
a)
voltaic
b)
electrolytic
2.
Calculate the standard cell potential.
3Mg  + 2Al3+ --> 2Al  + 3Mg2+
a)
+0.71 V
b)
-0.71 V
3.
Atoms of which element can most easily be oxidized?
a)
Copper
b)
Zinc
c)
Iron
d)
Calcium
4.

Calculate the standard cell potential cell in the following:

Zn / Zn2+ // Pb2+ / Pb

a)

+0.89 V

b)

+ 0.63 V

c)

- 0.89 V

d)

- 0.63 V

5.
The electrolysis of molten sodium chloride produces:
a)
hydrochloric acid
b)
sodium metal and chlorine gas
c)
chlorine gas and aqueous sodium hydroxide
d)
glucose
6.
Reactions in voltaic cells are
a)
spontaneous, redox reactions
b)
non-spontaneous, redox reactions
c)
spontaneous, non-redox reactions
d)
non-spontaneous, non-redox reactions
7.
Which of the following is not a similarity between voltaic and electrolytic cells?
a)
electrons flow from anode to cathode
b)
reduction occurs at cathode
c)
oxidation occurs at anode
d)
charges on anode and cathode are the same
8.
If the cell potential is negative, the reaction is?
a)
 a success
b)
spontaneous
c)
not spontaneous
9.
The cell potential of a spontaneous reaction is
a)
positive
b)
negative
10.

Which of the following statements is true in electrochemistry?

a)

a) In electrolytic cells, electricity is produced by conducting appropriate redox reactions

b)

b) In electrolytic cells, electricity is produced by conducting appropriate redox reactions

c)

c) In electrochemical cells, electric energy is converted into mechanical energy

d)

d) In electrolytic cells, electric energy is converted into chemical energy

11.

A salt bridge is required to measure the cell potential of an electrochemical cell. The function of the salt bridge is

a)

a) to provide large surface area for reactions to occur

b)

b) to allow electrons to flow through from one cell to another cell

c)

c) to allow ions to pass through and to maintain the ionic balance

d)

d) to increase the voltage of the electrochemical cell

12.

The electrochemical reactions in Rechargeable batteries are

a)

a) Non-reversible in nature

b)

b) Explosive in nature

c)

c) Reversible in nature

d)

d) Highly endothermic but irreversible in nature

13.

Which of the following statements applies to the change in mass of the electrodes involved in this electrochemical cell?

a)

Electrode A is the anode and it gains mass

since metal ions are being converted to metal

atoms which often adhere to the electrode.

b)

Electrode B is the anode and it gains mass

since metal ions are being converted to metal

atoms which often adhere to the electrode.

c)

Electrode A is the cathode and it gains mass since metal ions are being converted to metal atoms which often adhere to the electrode.

d)

Electrode B is the cathode and it gains mass since metal ions are

being converted to metal atoms which often adhere to the electrode.

14.

Which of the following best describes this electrochemical cell?

a)

Electrode A is the anode since anions are present in its half-cell and the current flows from cathode to anode.

b)

Electrode C is the cathode since cations are present in its half-cell and the current flows from anode to cathode.

c)

Electrode A is the anode and Electrode C is the cathode since the current always flows from cathode to anode.

d)

Electrode C is the anode and Electrode A is the cathode since the current always flows from anode to cathode.

15.
What is oxidation number of Cr in Cr2O72-?
a)
-2
b)
+2
c)
+6
d)
+12
16.
What is oxidation number of Fe in FeO ?
a)
+2
b)
-2
c)
0
d)
+1
17.
Which substance is reduced in the following reaction? 
NaOH + Li --> LiOH + Na
a)
Li
b)
Na
c)
O
d)
H
18.
Which of the following is the balanced half -reaction for the oxidation of Cu to Cu+2?
a)
Cu   --> Cu+2
b)
Cu + 2 e-   --> Cu+2
c)
Cu  --> Cu+2  + 2 e-
d)
Cu - 2e-  --> Cu+2
19.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
20.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
21.
Oxygen always has an oxidation number of...
a)
-1
b)
1
c)
2
d)
-2
22.
What is oxidation number of H in H2O?
a)
0
b)
-2
c)
-1
d)
+1
23.
What is the oxidation number of N in NO2-?
a)
-3
b)
+4
c)
-2
d)
+3
24.
What is oxidation number of O in O2 ?
a)
0
b)
-2
c)
+1
d)
+2
25.
What coefficient would Fe+2 have in the following reaction?
___ Al + ___ Fe+2 → ___ Al+3 + ___ Fe
a)
1
b)
2
c)
3
d)
6
26.
A group of cells that are connected together
a)
anode
b)
battery
c)
salt bridge
d)
half cell
27.
The electrode at which reduction occurs
a)
cathode
b)
anode
c)
salt bridge
d)
electrode
28.
A conductor in a circuit that carries electrons to or from a substance other than a metal.
a)
electrode
b)
battery
c)
salt bridge
d)
half cell
29.
Which of the following is true for an electrolytic cell?
a)
changes electrical energy into chemical energy.
b)
used in electroplating
c)
uses an electricity to make a nonspontaneous reaction go
d)
all of the above
30.
What does the double line mean?
Zn/Zn+2 // Cu+2/Cu
a)
anode
b)
cathode
c)
salt bridge
d)
substance in contact
31.

What is an electrolyte?

a)

The liquid part of the electrochemical cell

b)

The metal part of the electrochemical cell

c)

The part that measures the voltage in an electrochemical cell

32.

Which change in oxidation number indicates oxidation?

a)

–1 to +2

b)

–1 to –2

c)

+2 to –3

d)

+3 to +2

33.

What is the oxidation number of sulfur in Na2S2O3?

a)

-1

b)

+2

c)

+6

d)

+4

34.

Which species is oxidized when the switch is closed?

a)

Mg (s)

b)

Mg+2 (aq)

c)

Ag (s)

d)

Ag+(aq)

35.

Which is a redox reaction?

a)

Mg + 2 HCl --> MgCl2 + H2

b)

Mg(OH)2 + 2 HCl --> MgCl2 + 2 H2O

c)

Mg2+ (aq) + 2 OH– (aq) --> Mg(OH)2

d)

MgCl2 + 6 H2O --> MgCl2•6 H2O

36.

In the following cell diagram, which substance will be oxidized?

a)

Fe

b)

Fe2+

c)

Cu

d)

Cu2+

37.

In the following cell diagram, which substance will be reduced?

a)

Fe

b)

Fe2+

c)

Cu

d)

Cu2+

38.

In the following cell diagram, which substance will be the anode?

a)

Fe

b)

Fe2+

c)

Cu

d)

Cu2+

39.

In the following cell diagram, which substance will be the cathode?

a)

Fe

b)

Fe2+

c)

Cu

d)

Cu2+

40.

Using the following cell diagram, what is the correct cell notation?

a)

Fe/Fe2+//Cu2+/Cu

b)

Cu2+/Cu//Fe2+/Fe

c)

Fe2+/Fe//Cu/Cu2+

d)

Cu/Cu2+//Fe/Fe2+

41.

Using the following cell diagram, what would be the cell potential?

a)

-0.78 V

b)

+0.78V

c)

-0.60 V

d)

+0.60V

42.

Is the following spontaneous or non-spontaneous? Ag/Ag+//Al3+/Al

a)

spontaneous

b)

non-spontaneous

43.

Is the following spontaneous or non-spontaneous?

Na + Au3+ --> Au + Na+

a)

spontaneous

b)

non-spontaneous

44.

What is the correct balanced overall cell reaction for:

Mg/Mg2+//Au3+/Au

a)

2Mg + 3Au3+ --> 2Mg2+ + 3Au

b)

3Mg + 2Au3+ --> 3Mg2+ + 2Au

c)

3Mg2+ + 2Au --> 3Mg + 2Au3+

d)

2Mg2+ + 3Au --> 2Mg + 3Au3+

45.

If you had a water tank made of iron, which substance would be best used for cathodic protection?

a)

cobalt

b)

gold

c)

copper

d)

magnesium

46.

Which reactant pair will result in a spontaneous reaction?

a)

Au+ + Mg

b)

Hg + Fe3+

c)

Cr + Al3+

d)

Br2 + Au

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