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Worksheets

Exploring Electrochemistry Concepts

Total questions: 156

Worksheet time: 8hrs 36mins

Name
Class
Date
1.

What is an electrochemical cell?

a)

A device that only stores electrical energy.

b)

A type of battery that cannot be recharged.

c)

A machine that generates heat from chemical reactions.

d)

An electrochemical cell is a device that converts chemical energy into electrical energy or vice versa.

2.

Describe the components of a galvanic cell.

a)

A galvanic cell consists of a single electrode and a resistor.

b)

A galvanic cell is made up of a battery and a capacitor.

c)

A galvanic cell includes only a power source and a load.

d)

A galvanic cell includes two half-cells (anode and cathode), electrodes, electrolytes, and a salt bridge.

3.

What is the function of the salt bridge in an electrochemical cell?

a)

To act as a barrier preventing ion flow between electrodes.

b)

To maintain electrical neutrality and complete the circuit by allowing ion flow.

c)

To generate electricity directly without any ion movement.

d)

To increase the voltage output of the cell.

4.

Define oxidation and reduction in the context of redox reactions.

a)

Oxidation is the gain of protons; reduction is the loss of protons.

b)

Oxidation is the loss of mass; reduction is the gain of mass.

c)

Oxidation is the loss of electrons; reduction is the gain of electrons.

d)

Oxidation and reduction are both processes that involve the transfer of heat.

5.

What is the role of electrons in redox reactions?

a)

Electrons are not involved in chemical reactions.

b)

Electrons are produced during combustion reactions.

c)

Electrons are only involved in ionic bonding.

d)

Electrons are transferred between substances, facilitating oxidation and reduction.

6.

How do you identify the oxidizing and reducing agents in a reaction?

a)

The oxidizing agent is the substance that loses electrons.

b)

The oxidizing agent is the substance that gains electrons, and the reducing agent is the substance that loses electrons.

c)

Both agents are always the same substance in a reaction.

d)

The reducing agent is the substance that gains protons.

7.

What is the Nernst equation used for?

a)

To determine the temperature of a chemical reaction.

b)

To measure the concentration of a solution.

c)

To calculate the mass of reactants in a reaction.

d)

The Nernst equation is used to calculate the cell potential of an electrochemical cell under non-standard conditions.

8.

How does temperature affect the cell potential according to the Nernst equation?

a)

Temperature affects cell potential by influencing the Nernst equation, where higher temperatures can increase or decrease the potential depending on the reaction.

b)

Temperature has no effect on cell potential.

c)

Cell potential is only affected by concentration, not temperature.

d)

Higher temperatures always decrease cell potential.

9.

What is the standard electrode potential?

a)

The standard electrode potential is the temperature at which a reaction occurs.

b)

The standard electrode potential measures the concentration of ions in a solution.

c)

The standard electrode potential is the mass of the reactants involved in a reaction.

d)

The standard electrode potential is the voltage associated with a half-cell reaction at standard conditions.

10.

How do standard electrode potentials relate to the spontaneity of a reaction?

a)

A negative cell potential guarantees a reaction will occur.

b)

Standard electrode potentials have no effect on reaction rates.

c)

Standard electrode potentials help determine the spontaneity of a reaction; a positive cell potential indicates spontaneity.

d)

Standard electrode potentials only apply to gas-phase reactions.

11.

Explain the process of electrolysis.

a)

Electrolysis is the process of using electrical energy to drive a chemical reaction, typically involving the decomposition of an electrolyte.

b)

Electrolysis is the process of using light energy to decompose water.

c)

Electrolysis involves mixing chemicals to create a reaction without electricity.

d)

Electrolysis is a method of heating substances to high temperatures.

12.

What are the products of electrolysis of water?

a)

Hydrogen and Oxygen

b)

Methane and Ammonia

c)

Hydrogen Peroxide and Water

d)

Nitrogen and Carbon Dioxide

13.

What factors affect the efficiency of electrolysis?

a)

Factors affecting the efficiency of electrolysis include electrolyte type, concentration, temperature, applied voltage, electrode surface area, and electrode material.

b)

Type of light used during electrolysis

c)

Time of day when electrolysis is performed

d)

Size of the container holding the electrolyte

14.

How is Faraday's law related to electrolysis?

a)

Electrolysis is unrelated to any physical laws.

b)

Faraday's law only applies to magnetic fields, not electrolysis.

c)

Faraday's law quantifies the relationship between electric charge and the amount of substance transformed during electrolysis.

d)

Faraday's law states that electric charge has no effect on electrolysis.

15.

What is the difference between an electrolytic cell and a galvanic cell?

a)

Electrolytic cells require external energy; galvanic cells produce energy from spontaneous reactions.

b)

Galvanic cells are used for electrolysis; electrolytic cells are for energy production.

c)

Electrolytic cells generate energy; galvanic cells require energy.

d)

Both cells operate without any external energy source.

16.

How can you calculate the cell potential using standard electrode potentials?

a)

E_cell = E_anode / E_cathode

b)

E_cell = E_cathode * E_anode

c)

E_cell = E_cathode - E_anode

d)

E_cell = E_anode + E_cathode

17.

What is the significance of the SHE (Standard Hydrogen Electrode)?

a)

The SHE is used to measure temperature changes in reactions.

b)

The SHE is significant for determining the pH of solutions.

c)

The SHE is significant as a reference electrode for measuring standard electrode potentials.

d)

The SHE is a type of galvanic cell used for energy storage.

18.

Describe a practical application of electrochemical cells.

a)

Water purification systems.

b)

Batteries used in portable electronic devices.

c)

Thermal insulation materials.

d)

Solar panels for energy conversion.

19.

What is the relationship between Gibbs free energy and cell potential?

a)

Gibbs free energy is directly proportional to cell potential.

b)

Gibbs free energy is inversely related to cell potential; a negative ΔG indicates a positive cell potential.

c)

A positive ΔG indicates a negative cell potential.

d)

Cell potential has no relation to Gibbs free energy.

20.

How do concentration cells operate?

a)

Concentration cells produce electricity by mixing two different metals.

b)

Concentration cells require a constant temperature to function properly.

c)

Concentration cells generate electricity from the difference in ion concentration between two solutions.

d)

Concentration cells operate by using solar energy to generate electricity.

21.

Faraday's law of electrolytic cell

4 lines
22.

Diagram shows an electrolysis of dilute sulphuric acid.

What could be gas X and the half-equation occurring at the cathode?

a)

Carbon dioxide, C + O2 → CO2

b)

Hydrogen, 2H+ + 2e —>H2

c)

Oxygen, 4OH- → H2O + O2 + 4e-

d)

Sulphur dioxide, SO4 2- → SO2 + O2 + 2e-

23.

Which of the following reactions shows that copper is oxidized?

a)

Reaction of magnesium with copper (II)

oxide

b)

Reaction of copper with silver nitrate solution

c)

Electrolysis of copper (II) nitrate

solution by using carbon nitrate

d)

Voltaic cell with copper and magnesium

electrodes in dilute sulphuric acid

24.

Table shows the results of the electrolysis of molten lead (II) bromide.


The ammeter only shows reading when solid lead (II) bromide, PbBr2 is completely melted. Which of the following explains the observation?

a)

Bromide ions receive electrons to form bromine gas

b)

Lead (II) ions donate electrons to produce lead metal

c)

In the solid state, bromide and lead (II) ions are in fixed position

d)

Electrical conductivity occurs throughout

the whole experiment

25.

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

26.

In electrolysis, particles which move towards cathode are called

a)

anions

b)

cations

c)

photons

d)

positrons

27.

In electrochemical cell Anode is of which charge

a)

–ve

b)

+ve

c)

No charge

d)

Both charge

28.

When aqueous copper(II) chloride solution is electrolysed using copper electrodes, the half-equation for the reaction that occurs at the anode is

a)

Cu2+ + 2e -------> Cu

b)

Cu --------> Cu2+ + 2e

c)

2Cl- --------> Cl2 + 2e

d)

4OH- --------> 2H2O + O2 + 4e

29.

What are the cations present in zinc sulphate solution?

a)

Zn2+

b)

Zn2+, SO42

c)

Zn2+ , H+

d)

OH- , SO42-

30.

Which metal is the negative electrode?

Zn/Zn2+ // Cu2+/Cu

a)

zinc

b)

copper

31.

Galvanic cells convert

a)

mechanical energy in to electrical energy

b)

potential energy in to electrical energy

c)

electrical energy in to chemical energy

d)

chemical energy in to electrical energy

32.

Which of the species strong oxidizing agent?


Cl2(g) + 2e → 2Cl-(aq) Eocell = + 1.36 V

Cu2+(aq) + 2e → Cu(s) Eocell = + 0.34 V

Ni2+(aq) + 2e → Ni(s) Eocell = – 0.25 V

Ca2+(aq) + 2e → Ca(s) Eocell = – 2.87 V

a)

Cl2(g)

b)

Cu2+(aq)

c)

Ni2+(aq)

d)

Ca2+(aq)

33.

Which is correct to write cell notation

Anode: Zn

Cathode: Ni

a)

Zn2+ (aq,1M) / Zn (s) // Ni (s) / Ni2+ (aq,1M)

b)

Zn (s) /Zn2+ (aq,1M) // Ni2+ (aq,1M) / Ni (s)

c)

Zn2+ (s,1M) / Zn (aq) // Ni (aq) / Ni2+ (s,1M)

d)

Zn (aq) /Zn2+ (s,1M) // Ni2+ (s,1M) / Ni (aq)

34.

Calculate standard cell potential for this equation:


Zn2+(aq) + 2e → Zn(s) Eº = – 0.76 V

Cd2+(aq) + 2e → Cd(s) Eº = – 0.40 V

a)

Eocell = -0.36 V

b)

Eocell = -1.16 V

c)

Eocell = +1.16 V

d)

Eocell = +0.36 V

35.

One half-cell in a voltaic cell is constructed from a copper wire dipped into a 4.8 x 10 -3 M Solution of Cu(NO3)2. The other half-cell consist of zinc electrode in a 0.40 M Solution Zn(NO3)2. Calculate the Cell potential.

---

Cu2+(aq) (4.8 x 10 -3 M) + 2e- ---> Cu(s), if [Eored=0.337 V]

Zn2+(aq) (0.40 M) + 2e- ---> Zn(s), if [Eored= - 0.763 V]

---

Just the number value and the UNIT

(a)  

36.

In the cell notation;

one vertical line: denotes PHASE BOUNDARY

two vertical line: denotes (a)  

(two words, ANSWER IN ALL CAPS)

37.

How many participating electrons in the redox reaction of Fe2++Cr2O2-7 ---> Fe3++Cr3+? (Just the number)

(a)  

38.

How many participating electrons in the redox reaction of MnO-4 +I- ---> MnO2 + I2? (Just the number)

(a)  

39.

In the reaction of Cu(s) + Ni2+(aq) ---> Ni (s) + Cu2+(aq), the ________ undergoes reduction reaction.

a)

Copper

b)

Nickel

40.

Is it possible for a cell potential to have NEGATIVE sign?

a)

NO

b)

YES

41.

How many electrons is needed to transform Fe2+ ion to solid state?

a)

1

b)

2

c)

3

d)

4

42.

In a galvanic cell, it is an electrode where the oxidation happens?

a)

Cathode Electrode

b)

Anode Electrode

43.

A chemical species in an electrochemical reaction that GAINS electrons undergoes _________.

a)

Oxidation Reaction

b)

Reduction Reaction

44.

A chemical species in an electrochemical reaction that LOSSES electrons undergoes _________.

a)

Oxidation Reaction

b)

Reduction Reaction

45.

Which of the following statement is false

a)

flow of ions takes place in both direction

b)

conductivity of electrolyte is generally low

c)

electrolysis involves physical changes

d)

flow of electrons is unidirectional

46.

Electronic conduction is due to flow of

a)

Protons

b)

Electrons

c)

Neutrons

d)

Ions

47.

Electrochemistry deals with

a)

electric energy

b)

chemical energy

c)

only a

d)

both a & b

48.

In the reaction of Cu(s) + Ni2+(aq) ---> Ni (s) + Cu2+(aq), the ________ undergoes oxidation reaction.

a)

Copper

b)

Nickel

49.

True or False, is a negative sign of delta G a favorable answer that indicates spontaneity?

a)

TRUE

b)

FALSE

50.

Applications of Kohlrausch’s law

a)

Determination of Dissociation constant

b)

Degree of dissociation

c)

Solubility of sparingly soluble salts

d)

All the above

51.

EO represents

a)

Single electrode potential

b)

Standard electrode potential

c)

Standard hydrogen electrode

d)

None

52.

In electrochemical cell, oxidation takes place at

a)

Right

b)

Left

c)

Top

d)

Bottom

53.

In electrochemical cell, reduction takes place at

a)

Right

b)

Left

c)

Top

d)

Bottom

54.
Which direction do the electrons flow in wire X and which metal is oxidized?
a)
A
b)
B
c)
C
d)
D
55.
Which statement is correct when the cell produces electricity?
a)
Magnesium atoms lose electrons
b)
Mass of the iron electrode decreases.
c)
Electrons flow from the iron half-cell to the magnesium half-cell.
d)
Negative ion flow from magnesium half-cell to iron half-cell
56.
Oxidation happens at the
a)
anode
b)
cathode
c)
salt bridge
d)
voltmeter
57.

Reactions in galvanic/voltaic cells are

a)
spontaneous, redox reactions
b)
non-spontaneous, redox reactions
c)
spontaneous, non-redox reactions
d)
non-spontaneous, non-redox reactions
58.
In which direction does electricity flow in a voltaic cell (battery)?
a)
Electrons flow from the cathode to the anode
b)
Electrons flow from left to right
c)
Electrons flow from anode to cathode
d)
Electrons flow from right to left
59.
Metal A is more reactive than metal B. Which statement is correct?
a)
Electrons flow in the external circuit from A to B
b)
Positive ions flow through salt bridge from A to B
c)
Positive ions flow in external circuit from B to A.
d)
Electrons flow through salt bridge from B to A
60.
What is the function of Y in cell below?
a)

To maintain the excess buildup of charges in the electrolyte

b)
To allow flow of electrons between both cells
c)

To allow ions to move from one half cell to the other

d)
To connect both half cells
61.
Below shows a cell diagram for voltaic cell. Which of the following is FALSE?
a)
Electrons flow from anode to cathode
b)
Oxidation happens in anode
c)
Copper undergo reduction to form copper ions
d)
Zinc undergo oxidation to form Zinc ions
62.
Oxidation happens at the
a)
anode
b)
cathode
c)
salt bridge
d)
voltmeter
63.
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
64.
What reaction occurs at the anode?
a)
Ag+ + e- →Ag
b)
Ag → Ag+ + e-
c)
Ni2+ + 2e- → Ni
d)
Ni → Ni2+ + 2e-
65.

_______ is the reference electrode that can be used as an anode or a cathode depends on the half-cell to with it is coupled.

a)

Standard electrode potential

b)

Standard hydrogen electrode

c)

Standard cell potential

d)

Electrode potential

66.

Three factors affecting the selection of species to be discharged at electrodes    except..

a)

Standard reduction potential of the species

b)

Concentration of the species

c)

Nature of electrodes (active or inert)

d)

Mass of the species

67.
A student decided to silver-plate a locker key using the apparatus shown. In this cell, the key is the
a)
anode and is connected to the positive terminal of the power supply
b)
anode and is connected to the negative terminal of the power supply
c)
cathode and is connected to the positive terminal of the power supply
d)
cathode and is connected to the negative terminal of the power supply
68.

Reactions in electrolytic cells are

a)

spontaneous, redox reactions

b)

non-spontaneous, redox reactions

c)

spontaneous, non-redox reactions

d)

non-spontaneous, non-redox reactions

69.

The method of coating metals by immersing the metals in a liquid and then passing an electric current through the liquid is called ________

a)

Electrolysis

b)

Electroplating

c)

Electropalting

d)

Electroplation

70.

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

71.

Which of the following is NOT equal to 1 Faraday?

a)

96500C

b)

1 mole of electron

c)

one second

72.

how much charge is required to reduce 1 mol of Na+ into Na?

a)

2F

b)

3F

c)

2 X 96500 c

d)

96500 c

73.

how much charge is required to reduce 1 mol of Cu+2 into Cu?

a)

1 c

b)

2 c

c)

1F

d)

2F

74.

Given the standard electrode potentials,

K+/K = −2.93V, Ag+/Ag = 0.80V,

Hg2+/Hg = 0.79V

Mg2+/Mg = −2.37 V, Cr3+/Cr = − 0.74V

their increasing order of reducing power.

a)

K<Mg<Cr<Hg<Ag

b)

Ag >Hg > Cr > Mg > K

c)

Ag < Hg < Cr < Mg < K

d)

K>Mg>Cr>Hg>Ag

75.

Nernst equation FOR (i) Mg(s) | Mg2+(0.001M) || Al3+(0.0001 M) | Al(s)

a)

ECELL=E0CELL-0.0591/6 log[Mg2+]3/[Al3+]2

b)

ECELL=E0CELL-0.0591/6 log[Al3+]2/[Mg2+]3

c)

ECELL=E0CELL+0.0591/3 log[Mg2+]3/[Al3+]2

d)

ECELL=E0CELL-0.0591/3 log[Mg2+] /[Al3+]

76.

Conductivity always ____________ with a decrease in concentration

a)

decreases

b)

increases

c)

remain same

d)

irregular for weak and strong

77.

How much charge in Faraday is required for the following reductions:

1 mol of Al3+ to Al.

a)

1F

b)

2F

c)

3F

d)

4F

78.

conductivity of a solution decrease with dilution DUE TO

a)

The number of ionsper unit volume (responsible for carrying current) increases

b)

The number of ionsper unit volume (responsible for carrying current) decreases

c)

The number of ionsper unit volume (responsible for carrying current) remains same

d)

none

79.

molar conductivity of NH4OH increases sharply at infinite dilution due to

a)

decrease in dissociation

b)

increase in dissociation

c)

increase in association

d)

decrease in association

80.

Which of the following is the SI unit of conductivity.

a)

S m-1

b)

S m2 mol-1

c)

S m2 mol

d)

S m2 mol-2

81.

Which of the following is the SI unit of molar conductivity.

a)

S m-1 mol-1

b)

S m mol-1

c)

S m2 mol-1

d)

S m2 mol-2

82.

The value of Λm0\Lambda m^0  of CaCl2 is ------------.        given:  λm0(Ca2+=119.0) and λm0(Cl−=76.3)\lambda m^0\left(Ca^{2+}=119.0\right)\ and\ \lambda m^0\left(Cl^-=76.3\right)  

a)

271.6

b)

195.3

c)

314,3

d)

390.6

83.

which of the following is not correct

a)

G* = Rk

b)

G* = l/A

c)

G* = Gk

d)

k = GG*

84.

What is the oxidation state for a lead atom?

a)

2+

b)

4+

c)

0

d)

2-

85.

What is the oxidation number of carbon in H2CO3(aq)?

a)

4-

b)

2+

c)

2-

d)

4+

86.

When an electrochemical cell is operating, it is

a)

approaching equilibrium

b)

using external energy

c)

undergoing oxidation, only

d)

undergoing reduction, only

87.

Which statement best describes how a salt bridge maintains electrical neutrality in the half-cells of an electrochemical cell?

a)

It prevents the migration of electrons.

b)

It prevents the reaction from occurring spontaneously.

c)

It permits the migration of ions.

d)

It allows for the reaction from occurring spontaneously.

88.
Which of the following half reactions correctly represents a reduction half reaction?
a)
Fe →Fe2+ + 2e-
b)
Pb4+ + 2e- →Pb2+
c)
2O-2 →O2 + 4e-
d)
Fe + 3e- →Fe3+
89.
Which direction do the electrons flow in wire X and which metal is oxidized?
a)
A
b)
B
c)
C
d)
D
90.
In which direction does electricity flow in a voltaic cell (battery)?
a)
Electrons flow from the cathode to the anode
b)
Electrons flow from left to right
c)
Electrons flow from anode to cathode
d)
Electrons flow from right to left
91.
What reaction occurs at the anode?
a)
Ag+ + e- →Ag
b)
Ag → Ag+ + e-
c)
Ni2+ + 2e- → Ni
d)
Ni → Ni2+ + 2e-
92.
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
93.
Oxidation happens at the
a)
anode
b)
cathode
c)
salt bridge
d)
voltmeter
94.
Reduction happens at the 
a)
anode
b)
cathode
c)
salt bridge
d)
voltmeter
95.
What happens to Cr3+ ion when it is converted to CrO42–
a)
Oxidation number decreases and it undergo reduction
b)
Oxidation number decreases and it undergo oxidation
c)
Oxidation number increases and it undergo reduction
d)
Oxidation number increases and it undergo oxidation
96.
Which change does nitrogen undergo oxidation?
a)
A
b)
B
c)
C
d)
D
97.
Which are examples of reduction?
a)
I and II
b)
I and III
c)
II and III
d)
I, II and III
98.
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
99.
Is calcium oxidized or reduced in the following reaction? 
2CaO--> 2Ca + O2
a)
Oxidized
b)
Reduced
100.
How would you write the electrons in the reaction O2 --> O2-2 ?
a)
+2e- on the products
b)
+2e- on the reactants
c)
+e- on the products
d)
+e- on the reactants
101.
Another name for a "oxidation-reduction" reaction is
a)
chemical reaction
b)
neutralization reaction
c)
redox reaction
d)
nuclear reaction
102.
     In the reaction Zn + H2O --> ZnO2 + H2
 which element, if any, is oxidized? 
a)
Zinc
b)
Hydrogen
c)
Oxygen
d)
None
103.
Which of the following elements does NOT have an oxidation number of +2?
a)
Ca
b)
Sr
c)
K
d)
Ba
104.
What is oxidation number of O in O2 ?
a)
0
b)
-2
c)
+1
d)
+2
105.
What is oxidation number of P in K3PO4?
a)
+1
b)
+5
c)
-2
d)
0
106.
What is oxidation number of Cr in Cr2O72-?
a)
-2
b)
+2
c)
+6
d)
+12
107.
What is the oxidation number of Fe in FeO?
a)
+1
b)
-1
c)
+2
d)
-2
108.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
109.

In a galvanic cell with the following cell notation:

 ∣Ni(s)∣Ni+2(aq)∥Co+2(aq)∣Co(s)∣\left|Ni\left(s\right)\right|Ni^{+2}\left(aq\right)\parallel Co^{+2}\left(aq\right)\left|Co\left(s\right)\right|  

Which of the following is true?

a)

Ni is being reduced

b)

 Co+2 is being oxidizedCo^{+2}\ is\ being\ oxidized  

c)

Energy will be added to operate this cell.

d)

This cell operated spontaneously

110.
What unit of measurement do we use to measure electrical potential?
a)
Watts
b)
Volts
c)
Amps
d)
Ohms
111.

An electrolytic cell uses electrical energy to drive

a)

chemical reaction

b)

physical reaction

c)

no reaction

d)

none of above

112.

Galvanic cells convert

a)

mechanical energy in to electrical energy

b)

potential energy in to electrical energy

c)

electrical energy in to chemical energy

d)

chemical energy in to electrical energy

113.

Pb + 2Ag+ → Pb+2 + 2Ag


The chemical species being reduced is

a)

Ag

b)

Pb

c)

Pb+2

d)

Ag+

114.

Oxidation-reduction reactions occur because of the competition between particles for

a)

electrons

b)

positrons

c)

protons

d)

neutrons

115.

The reaction 2NaCl → 2Na + Cl2 is an example of

a)

a reduction reaction, only

b)

both an oxidation and reduction reaction

c)

an oxidation reaction, only

d)

neither an oxidation nor a reduction reaction

116.

An oxidizing agent will

a)

increase in mass

b)

lose electrons

c)

be reduced

d)

increase in oxidation number

117.

Electrochemistry is

a)

Study of electron in atom

b)

Study of electricity in molecules

c)

The relationship between chemical reactions and electricity

d)

the study of electrons moving from one a tom to another

118.

Diagram shows an apparatus set-up for a chemical cell. What can you observed from this experiment?

a)

Hydrogen gas is liberated at the copper plate

b)

Magnesium electrode becomes thinner

c)

Colourless solution turns to brown

d)

Electron flows from magnesium to the copper plate

119.

Diagram shows an electrolysis of dilute sulphuric acid.

What could be gas X and the half-equation occurring at the cathode?

a)

Carbon dioxide, C + O2 → CO2

b)

Hydrogen, 2H+ + 2e- → H2

c)

Oxygen, 4OH- → H2O + O2 + 4e-

d)

Sulphur dioxide, SO4 2- → SO2 + O2 + 2e-

120.

Which of the following reactions shows that copper is oxidized?

a)

Reaction of magnesium with copper (II) oxide

b)

Reaction of copper with silver nitrate solution

c)

Electrolysis of copper (II) nitrate solution by using carbon nitrate

d)

Voltaic cell with copper and magnesium electrodes in dilute sulphuric acid

121.

Table shows the results of the electrolysis of molten lead (II) bromide.


The ammeter only shows reading when solid lead (II) bromide, PbBr2 is completely melted. Which of the following explains the observation?

a)

Bromide ions receive electrons to form bromine gas

b)

Lead (II) ions donate electrons to produce lead metal

c)

In the solid state, bromide and lead (II) ions are held in a lattice

d)

Electrical conductivity occurs throughout

the whole experiment

122.

Molten X is electrolysed using carbon electrodes. After 10 minutes, a brown solid is deposited on the cathode and a brown gas is released at the anode. What is molten X?

a)

Lead(II) chloride

b)

Lead(II) bromide

c)

Copper(II) chloride

d)

Copper(II) bromide

123.

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

124.

Diagram shows the electrolysis of concentrated copper(II) chloride solution using carbon as electrodes.

Which of the followings is the correct half equations represents the reactions at the anode?

a)

4OH- → 2H2O + O2 + 4e

b)

2Cl- → Cl2 + 2e

c)

Cu → Cu2+ + 2e

d)

Cu2+ + 2e → Cu

125.

Table shows information about three chemical cells.

What is the possible potential difference of the chemical cell when metal Z is paired with W ?

a)

0.3 V

b)

1.2 V

c)

1.5 V

d)

2.1 V

126.

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

127.

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

128.

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-

129.

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

130.

Nernst equation for an electrode is based on the variation of electrode potential of an electrode with

a)

Temperature

b)

Concentration of electrolyte

c)

Both a & b

d)

Density of the electrodes

131.

At equilibrium

a)

Cell potential will be zero

b)

Equilibrium constant becomes equal to electrode potential

c)

Equilibrium constant becomes zero

d)

Cell potential becomes unity

132.

Galvanic cell converts

a)

Chemical energy into electrical energy

b)

Electrical energy into chemical energy

c)

a metal from its elemental form to combined form

d)

Electrolyte into individual ions

133.

Given the standard reduction potentials, Eo of iron is -0.44V and Eo of oxygen is 1.23V.

what will be the emf of the cell?

a)

-0.79V

b)

-1.67V

c)

1.67V

d)

0.79V

134.

Consider the galvanic cell reaction Zn (s) + Cu2+ (aq) → Cu (s) + Zn2+ (aq) When the cell is running spontaneously, which is the only true statement?

a)

The copper electrode loses mass and the zinc electrode is the cathode.

b)

The copper electrode gains mass and the copper electrode is the cathode.

c)

The zinc electrode gains mass and the zinc electrode is the anode.

d)

The zinc electrode loses mass and the zinc electrode is the cathode.

135.

In a Galvanic Cell, the salt bridge...

a)

completes the circuit so that electrons can flow through the wire

b)

maintains charge balance

c)

is soaked in an unreactive electrolyte such as KNO3

d)

all of the above

136.

In a Galvanic cell, the cations in the salt bridge...

a)

flow the same way as the electrons flow in the wire

b)

flow the opposite way to the electron flow in the wire

c)

stay in the salt bridge

137.

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

138.

In a Galvanic cell, the electrons flow from the...

a)

anode to the cathode

b)

cathode to the anode

139.

In a Galvanic Cell, the anode is...

a)

positive

b)

negative

140.
Which statement is correct?
a)
Ca2+ can oxidize Ni
b)
Ni2+ can reduce Ca2+
c)
Fe3+ can oxidize Ni
d)
Fe3+ can reduce Ca2+
141.
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
142.
What is the equation and cell potential?
a)
2Al3+ + 3Ni → 2Al + 3Ni2+ EO = 1.89 V
b)
2Al + 3Ni2+ → 2Al3+ + 3Ni EO = 1.89 V
c)
2Al3+ + 3Ni → 2Al + 3Ni2+ EO = 1.43 V
d)
2Al + 3Ni2+ → 2Al3+ + 3Ni EO = 1.43 V
143.
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
144.
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)
145.
Calculate the cell potential of voltaic cell
a)
–1.60 V
b)
+1.60 V
c)
–3.12 V
d)
+3.12 V
146.
Calculate the cell potential of voltaic cell
a)
–1.51
b)
- 0.03
c)
+0.03
d)
+1.51
147.
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
148.

What is a cathode?

a)

It is the electrode where oxidation takes place.

b)

It is the electrode where reduction takes place.

c)

It is an aqueous solution containing an electrode.

d)

It is the salt bridge that connects half-cells.

149.

What is an anode?

a)

It is the electrode where oxidation takes place.

b)

It is the electrode where reduction takes place.

c)

It is an aqueous solution containing an electrode.

d)

It is the salt bridge that connects half-cells.

150.

What is a standard half-cell?

a)

It is one cell that comprises half of a whole battery.

b)

It is a cell containing only a metal bar with no aqueous ion solution.

c)

It is a cell containing only an aqueous ion solution and no metal bar.

d)

It is a cell that generates half of a volt of electricity.

151.

What is a galvanic (voltaic) cell?

a)

It is a cell that destroys electrons on one side and creates electrons on the other side.

b)

It is a cell that contains only one metal bar and one aqueous ion solution.

c)

It is a type of battery that drives a redox reaction when electricity is applied.

d)

It is a type of battery that generates an electrical current from redox reactions.

152.

What is an oxidizing agent?

a)

It is the species that gets reduced -- gains electrons.

b)

It is the species that gets oxidized -- loses electrons.

c)

It is the species that creates electrons.

d)

It is the species that loses electrons.

153.

What is a reducing agent?

a)

It is the species that gets reduced -- gains electrons.

b)

It is the species that gets oxidized -- loses electrons.

c)

It is the species that creates electrons.

d)

It is the species that destroys electrons.

154.

What is oxidation?

a)

It is the gain of electrons.

b)

It is the loss of electrons.

c)

It is the creation of electrons.

d)

It is the destruction of electrons.

155.

What is reduction?

a)

It is the gain of electrons.

b)

It is the loss of electrons.

c)

It is the creation of electrons.

d)

It is the destruction of electrons.

156.

What is a redox reaction?

a)

A reaction where both reactants get reduced.

b)

A reaction where both reactants get oxidized.

c)

A reaction that involves a transfer of electrons between reactants.

d)

A reaction that involves the combustion of at least one reactant.