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Electrochemisty - theory revision

Total questions: 60

Worksheet time: 45mins

Name
Class
Date
1.

Given their standard reduction potentials, which of the species is going to be oxidized?

Cu2+/Cu = 0.34V

Zn2+/Zn = -0.76V

a)

Cu

b)

Zn

c)

CuSO4

d)

ZnSO4

2.
An iron nail is put into a solution of copper nitrate, iron is above copper in the activity series of metals, what will happen?
a)
iron will be reduced
b)
bubbles of oxygen gas will form on iron nail
c)
the iron nail will become copper plated
d)
no reaction occurs
3.
If Al is above Co in the activity series of metals, which of the following will occur if Al metal is put into a solution of cobalt nitrate?
a)
a redox reaction takes place
b)
the Al strip dissolves
c)
the Al strip becomes coated with cobalt
d)
all of the above
4.

What occurs to the mass of copper electrode in the following reaction?

Zn/Zn2+ // Cu2+/Cu

a)

increases

b)

decreases

c)

remains the same

5.

Which metal is the negative electrode?

Zn/Zn2+ // Cu2+/Cu

a)

zinc

b)

copper

6.

What reaction occurs at the anode?

Ag+/Ag = 0.80V

Ni2+/Ni = -0.25V

a)

Ag+ + e- →Ag

b)

Ag → Ag+ + e-

c)

Ni2+ + 2e- → Ni

d)

Ni → Ni2+ + 2e-

7.

Conductivity always ____________ with a decrease in concentration

a)

decreases

b)

increases

c)

remain same

d)

irregular for weak and strong

8.

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.

9.

Diagram shows an electrolysis cell.

Which of the substances cause the bulb to light up when electricity passes through it?

a)

Ethanol

b)

Dilute ethanoic acid

c)

Solid lead(II) bromide

d)

Tetrachloromethane

10.

What are the products formed at the anode and the cathode during the electrolysis of molten magnesium oxide using carbon electrodes?

a)

Anode: Oxygen

Cathode: Magnesium

b)

Anode: Magnesium

Cathode: Oxygen

c)

Anode: Hydrogen

Cathode: Oxygen

d)

Anode: Oxygen

Cathode: Hydrogen

11.

Diagram

shows the apparatus set-up for the electrolysis of 1.0 mol dm -3 sodium chloride solution using carbon electrodes.Which of the following are the observation for the electrolysis process shown in Diagram?


a)

Grey solid deposited on electrode B

b)

Colourless gas is released at electrode B

c)

Carbon electrode A becomes thinner

d)

Greenish yellow gas is released at electrode A

12.
What unit of measurement do we use to measure electrical potential?
a)
Watts
b)
Volts
c)
Amps
d)
Ohms
13.
What are the features of a standard hydrogen electrode?
a)
I and II
b)
I and III
c)
II and III
d)
I, II and III
14.
Which represents reduction process occurring in standard hydrogen electrode?
a)
H2(g) → 2H+(aq) + 2e–
b)
H+(aq) + OH–(aq) → H2O(l)
c)
2H+(aq) + 2e– → H2(g)
d)
O2(g) + 4H+(aq) + 4e– → 2H2O(l)
15.
Which statement is correct about value of Eο?
a)
more positive value Eο, greater driving force for reduction
b)
more negative value Eο, greater driving force for reduction
c)
more positive value Eο, greater the rate of reaction
d)
more negative value Eο, greater the rate of reaction
16.
What happen when zinc is added to magnesium chloride?
a)
No reaction will take place
b)
Chlorine gas will be produced
c)
Magnesium metal will form
d)
Zinc chloride will form
17.
What is Eo for the following reaction?
a)
+0.85
b)
+0.51
c)
–1.53
d)
–1.87
18.
A galvanic cell was set up as shown. 
The standard redox potentials for these half-cells are:
Ag+(aq)  +  e- →  Ag(s);  E0 = 0.89 V
Ni2+(aq)  + 2e- →  Ni(s);  E0 = -0.23 V
In this cell:
a)
the silver electrode has positive polarity and the nickel electrode will corrode.
b)
the silver electrode has positive polarity and the silver electrode will corrode. 
c)
the silver electrode has negative polarity and the nickel electrode will corrode. 
d)
the silver electrode has negative polarity and the silver electrode will corrode.
19.

A disproportionation reaction occurs when a species M+ spontaneously undergoes simultaneous oxidation and reduction.


2M+(aq) → M2+(aq) + M(s)


The table contains E⦵ data for copper and mercury species.


Using these data, which one of the following can be predicted?

a)

Both Cu(I) and Hg(I) undergo disproportionation.

b)

Only Cu(I) undergoes disproportionation.

c)

Only Hg(I) undergoes disproportionation.

d)

Neither Cu(I) nor Hg(I) undergoes disproportionation.

20.

Why is Standard hydrogen electrode called as the primary reference electrode?

a)

a) It has a known output potential

b)

b) It has a constant output potential

c)

c) Its output potential is independent of the composition of the solution

d)

d) Its output potential is zero volts

21.

Given below is a diagram of a standard hydrogen electrode. Identify the unmarked component.

a)

a)Hydrogen at 1 atm

b)

b) Hydrogen at 10 atm

c)

c) Helium at 1 atm

d)

d) Helium at 10 atm

22.

In the list of standard electrode potentials, the strongest reducing agent is...

a)

Li

b)

Li+

c)

F2

d)

F-

23.

In a redox reaction, the oxidising agent... (choose two options)

a)

is oxidised

b)

is reduced

c)

increases its oxidation number

d)

decreases its oxidation number

24.

If an electrochemical reaction is spontaneous, what will Ecell be?

a)

positive

b)

negative

25.

What is the standard electrode which all other standard electrode potentials are measured against?

a)

helium

b)

hydrogen

c)

magnesium

d)

potassium

26.
A galvanic cell was set up from a Cl2/Cl- half-cell and a standard hydrogen electrode (SHE). It was found that the voltmeter reading was 1.36 V and the chlorine half-cell was the positively-charged electrode. Which statement about this galvanic cell is INCORRECT?
a)
Both of the electrodes should be made of platinum. 
b)
The chlorine half-cell is the anode. 
c)
As the cell operates, the pH of the solution in the SHE decreases. 
d)
The standard redox potential for the chlorine half-cell must be +1.36 V.
27.
In the ethanol fuel cell, ethanol is pumped in at one electrode and oxygen is pumped in at the other. The only products of the cell reaction are the same as those that would be produced if ethanol was burnt directly in excess air. What is the correct equation for the reaction at the anode, if an acidic electrolyte is used?
a)
O2(g) + 4H+(aq) + 4e-→  2H2O(l) 
b)
O2(g)+ 2H+(aq) +  2e- → 2H2O2(aq)
c)
C2H5OH(aq) + 3H2O(l) → 2CO2(g)  +  12H+(aq)  +  12e- 
d)
C2H5OH(aq) + 3H2O(l) → 2CO2(g)  + 11H+(aq) +  11e-
28.
The diagram below shows a hydrogen–oxygen fuel cell that is operating with an acidic electrolyte.
What is Gas X and what is the polarity of electrode N? 
a)
Hydrogen; positive
b)
Hydrogen; negative
c)
Oxygen; positive
d)
Oxygen; negative
29.
What is the key difference between a galvanic cell and a fuel cell? 
a)
Galvanic cells deliver direct current; fuel cells deliver alternating current. 
b)
Galvanic cells are essentially for energy storage; fuel cells work continuously. 
c)
Galvanic cells do not use gases as reactants; fuel cells only use gases. 
d)
Galvanic cells are not rechargeable; fuel cells are constantly recharged.
30.
In commercial galvanic cells, a separator is used instead of a salt bridge. Which of the following is NOT a property that the separator should possess? 
a)
Good conductor of electricity
b)
Will allow certain ions to migrate through it 
c)
Inert
d)
Low density
31.
Consider the galvanic cell given.
Which of the following deductions about this cell is correct?
a)
Oxidation is occurring in half-cell 2
b)
The positive electrode is in half-cell 2
c)
Oxidation is occurring in half-cell 1
d)
The negative electrode is in half-cell 1
32.

The potential developed due to gain of electrons

a)

Oxidation Potential

b)

Electrode potential

c)

Reduction Potential

d)

None

33.

The conductance of ions, present in one cubic centimeter of the solution.

a)

Ionic Conductance

b)

Specific Conductance

c)

Molar Conductance

d)

Equivalent conductance

34.

The electrodes used in chemical cell without transference in which the electrolyte is HCl are----------

a)

Hydrogen gas electrode and Cadmium electrode

b)

Hydrogen gas electrode and Copper electrode

c)

Hydrogen gas electrode and Silver - Silver Chloride electrode

d)

Hydrogen gas electrode and lead - lead Sulphate electrode

35.

The elimination of liquid junction potential in cell representation is indicated by ---------

a)

-ve sign

b)

+ve sign

c)

Vertical double line between two half cells

d)

Vertical single line between two half cells

36.

What does a half-cell consist of?

a)

two elements in two oxidation states

b)

two elements in the same oxidation state

c)

one element in two oxidation states

d)

one element in one oxidation state

37.

With dilution which of the following decreases

a)

Specific Conductance

b)

Molar Conductance

c)

Equivalent Conductance

d)

Resistance

38.
What is an electrolytic cell? 
a)
a cell that converts chemical energy into electrical energy 
b)
a cell that converts electrical energy into electrical energy 
c)
a cell that converts electrical energy into chemical energy 
d)
A cell that converts kinetic energy into potential energy. 
39.

If the conductivity and conductance of a solution is same then its cell constant is equal to

a)

1

b)

0

c)

10

d)

1000

40.

Which of the following factors is responsible for increase in equivalent conductivity in the case of weak electrolytes upon dilution?

a)

decrease in degree of dissociation with dilution

b)

increase in degree of dissociation with dilution

c)

decrease in inter-ionic effects upon dilution

d)

increase in inter-ionic effects upon dilution

41.

What is the standard solution used for determining cell constant?

a)

Potassium chloride

b)

Sodium chloride

c)

Potassium hydroxide

d)

Sodium hydroxide

42.

The principle of --------------- titration is based on the fact that during the titration, one of the ions is replaced by the other and invariably these two ions differ in the ionic conductivity with the result that conductivity of the solution varies during the course of titration.

a)

potentiometric

b)

conductometric

c)

polarographic

d)

gravimetric

43.

In redox titration, large quantities of acids and beases are used to complete reaction which masks the changes in conductance, hence in conductometric titration, redox titration

a)

Performed at high temperature

b)

Performed at cryogenic conditions

c)

Cannot be performed

d)

Performed using indicator solution

44.
Which curve is produced by the titration of a 0.1M weak base with 0.1M strong acid?
a)
A
b)
B
c)
C
d)
D
45.
Which acid base pair produce the titration curve shown below?
a)
HCI + KOH
b)
HCI + NH3
c)
CH3COOH + KOH
d)
CH3COOH + NH3
46.
A simplified diagram of the phosphoric acid fuel cell (PAFC), and their half-reactions are shown. The cell operates at 190oC using an electrolyte of liquid phosphoric acid.
During operation of the PAFC, electrode I is
a)
positively charged, and the pH near the electrode will increase
b)
positively charged, and the pH near the electrode will decrease
c)
negatively charged, and the pH near the electrode will increase
d)
negatively charged, and the pH near the electrode will decrease
47.
Methane gas is used as a fuel in an acidic fuel cell. The half-equation occurring at the anode will be
a)
O2(g) + 4H+(aq) + 4e- →2H2O(g)
b)
CH4(g) + 2H2O(g) → CO2(g) + 8H+ (aq) + 8e-
c)
CH4(g) + 4H+(g)→ CO2(g) + 4H2O(l)
d)
CO2(g) + 8H+(aq) + 8e- → CH4(g) + 2H2O(g)
48.

The storage battery generally used in electric power station is

a)

Nickel-cadmium battery

b)

Zinc carbon battery

c)

Lead-acid battery

d)

None of the above

49.

Electroplating is an industrial process where objects are coated by a thin layer of a nonreactive metal by electrolysis. What should be used as the cathode in this process?

a)

Graphite electrode

b)

The electroplating metal

c)

The object to be electroplated

d)

Magnesium ribbon

50.

If the fork is to be electroplated with silver metal, what electrolyte should be used?

a)

Molten silver chloride

b)

Aqueous silver nitrate

c)

Sodium chloride solution

d)

Copper(II) sulphate solution

51.

PbO2 means

a)

Lead dioxide

b)

Lead peroxide

c)

Lead sulfate

d)

Sponge lead

52.

When there is a higher acid concentration on the bottom of a battery then on the top, this is called...

a)

sulfation

b)

stratification

c)

concentration reduction

d)

acid redux

53.

When sulfuric acid crystals are deposited on battery plates, they reduce battery capacity. This is called...

a)

sulfation

b)

sulfur depletion

c)

capacity reduction

d)

sulfuric crystallization

54.

A battery with no load connected will still

discharge. This is called…

a)

depth of charge

b)

charge depletion

c)

self-discharge

d)

electrolyte deficieny

55.

lead -acid storage battery it contains of ____cells.

a)

1

b)

2

c)

4

d)

6

56.

A primary cell is a cell that...

a)

can only be used once

b)

can be recharged and used again

c)

is reusable

d)

is used again and again

57.

What is the equation at the anode for the discharge of a nickel cadmium cell?

a)

2NiO(OH) (s) + 2H2O (l) + 2e- → 2NiOH2 (s) + 2OH-

b)

Cd(s) + 2OH-(aq) → Cd(OH)2 + 2e-

c)

Cd(s) + 2H2O (l) → Cd(OH)(aq) + H2 (g)

d)

NiO(OH) (s) + 2OH-(aq) → Ni(OH)2 + 2e- + H2O (l)

58.

Which of the following is an advantage of lithium ion cells?

a)

High energy density and high discharge rates

b)

Charge quickly and have a high number of cycles

c)

High energy density and low discharge rate

d)

Cheap to make

59.

In an electrolytic cell between magnesium and zinc, which of the following will increase the Ecell?

a)

Increasing concentration of solid magnesium (whilst keeping all other concentrations the same).

b)

Increasing concentration of zinc ions getting oxidised (whilst keeping all other concentrations the same).

c)

Increasing concentration of magnesium ions (whilst keeping all other concentrations the same).

d)

Decreasing the temperature.

60.

What is a disadvantage of using a nickel cadmium battery?

a)

Expensive to produce.

b)

Known to cause electrical fires.

c)

Harmful to the environment after it is disposed.

d)

Overcharging leads to production of hydrogen gas, which can explode.

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