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Electrochemistry Test - 4

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Electrochemistry Test - 4

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Question 1
1 / -0

For a dilute solution of a strong electrolyte, which of the following facts is correct?

A
The graph between _m and c is linear.

B
The graph between log _m and c is linear.

C
The graph between _m and is linear.

D
The graph between log _m and log c is linear.
Question 2
1 / -0

Fundamental difference between an electrolytic cell and the galvanic cell is that in electrolytic cell

A
the free energy is supplied in the form of mechanical work done on the system by the outside world

B
in electrolytic cell the free enenrgy is supplied in the form of mechanical work done by the system on the outside world

C
the free energy decreases as work is done by the system on the outside world

D
he free energy is supplied in the form of electrical work done on the system by the outside world

Solution

In electrolytic cell electrical energy is converted into chemical energy. Here the electrical energy is used to drive redox reactions which have positive free energy and are non spontaneous
Question 3
1 / -0

Two half-cells have potentials – 0.44 V and 0.799 V, respectively. These two are coupled to make a galvanic cell. Which of the following statements is true?

A
Electrode of half-cell potential – 0.44 V acts as anode.

B
Electrode of half-cell potential – 0.44 V acts as cathode.

C
Electrode of half-cell potential 0.799 V acts as anode.

D
None of these
Question 4
1 / -0

Galvanic or a voltaic cell converts the chemical energy liberated during a redox reaction to

A
acoustic energy

B
electromagnetic energy

C
thermal energy

D
electrical energy

Solution

Galvanic cells convert chemical energy to electrical energy.
Question 5
1 / -0

Zinc/Silver oxide cell is used in electric watches.

Zn Zn²⁺ + 2e^-E⁰ = - 0.76 V

Ag₂O + H₂O + 2e^- 2Ag + 2OH^-E⁰ cell = 0.344 V

Find G⁰ in joules.

A
- 1.30 x 10⁶ J

B
- 2.13 x 10⁵ J

C
2.13 x 10⁷ J

D
1.30 x 10⁶ J
Question 6
1 / -0

Electrochemistry deals with the production of electricity from

A
energy released during spontaneous chemical reactions and the use of electrical energy to bring about non-spontaneous chemical transformations

B
nuclear energy and the use of heat energy to bring about non-spontaneous chemical transformations

C
energy released during spontaneous chemical reactions and the use of heat energy to bring about non-spontaneous chemical transformations

D
nuclear energy and the use of electrical energy to bring about non-spontaneous chemical transformations

Solution

Electrochemistry is branch of chemistry that deals with production of electricity from a redox chemical reaction or carrying out a non spontaneous reaction using electrical energy.
Question 7
1 / -0

The cell constant is defined as

A
l/a

B
a/l

C
l a

D
l²/a
Question 8
1 / -0

Which of the following statements is not true for a galvanic cell when written in an abbreviated form?

A
Left half electrode is the negative terminal.

B
Left half electrode is an anode.

C
Electrons are given out in the external circuit from the anode.

D
Electrons are given out in the external circuit from the cathode.
Question 9
1 / -0

Choose the correct statement from the following.

A
Conductivity of platinum metal increases on heating from 0^oC to 100^oC.

B
Aqueous NaCl is a better conductor at 50^oC than at 25^oC.

C
Conductivity of cane sugar solution increases with dilution.

D
Specific conductance of N/10 H₂SO₄ falls off with dilution.
Question 10
1 / -0

Zn (s) + Cl₂(1 atm) Zn²⁺ + 2Cl^-E^o_cell of the cell is 2.12 V. To increase E_cell,

A
[Zn²⁺] should be increased

B
[Zn²⁺] should be decreased

C
[Cl^-] should be decreased

D
should be decreased
Question 11
1 / -0

Which of the following statements is correct?

A
The equivalent conductance of both strong and weak electrolytes decreases with dilution.

B
The equivalent conductance of strong electrolytes increases with dilution, while that of weak electrolytes decreases with dilution.

C
The equivalent conductance of strong electrolytes decreases with dilution, while that of weak electrolytes increases with dilution.

D
The equivalent conductance of both strong and weak electrolytes increases with dilution.
Question 12
1 / -0

The potential of the cell Pt | H₂(g, 1 atm)H⁺ (0.01 M) || OH^–(10^–6 M)|H₂(g, 1 atm)| Pt at 298 K will be

A
– 0.236 V

B
0.236 V

C
– 0.472 V

D
0.472 V
Question 13
1 / -0

A solution is 0.1 M in each of Pb²⁺ and Fe²⁺ ions. If powders of lead and iron are added in this solution, which of the following facts comes out to be true?

A
More of Fe and Pb²⁺ ions are formed.

B
More of Pb and Fe²⁺ ions are formed.

C
Concentrations of Pb²⁺ and Fe²⁺ ions are increased.

D
Concentrations of Pb²⁺ and Fe²⁺ ions are decreased.
Question 14
1 / -0

A cell utilises the reaction Zn (s) + 2H⁺ (aq) Zn²⁺ (aq) + H₂ (g). Addition of H₂SO₄ to the cathode compartment will

A
lower E and shift equilibrium to the left

B
lower E and shift equilibrium to the right

C
increase E and shift equilibrium to the right

D
increase E only
Question 15
1 / -0

Two Faraday of electricity is passed through a solution of CuSO₄. The mass of copper deposited at the cathode is
(Atomic mass of Cu = 63.5 amu)

A
0 g

B
63.5 g

C
2 g

D
127 g
Question 16
1 / -0

The standard free energy change of the reaction Cu²⁺ + Sn(s) Cu(s) + Sn²⁺ (Given: E° = 0.48 V) is

A
– 31.8 kJmol^–1

B
– 62.1 kJmol^–1

C
– 79.2 kJmol^–1

D
– 92.64 kJmol^–1
Question 17
1 / -0

The unit of conductance is

A

B

C

D
Question 18
1 / -0

When a rod of metallic lead was added to 0.01 M solution of Co (en)₂²⁺, it was found that 68% of the cobalt complex was reduced to Co. (en)₃²⁺ by the lead. is - 0.126 V

Value of the equilibrium constant for the following reaction is:
Pb + 2Co (en)₃3+ Pb²⁺ + 2 Co(en)₃²⁺

A
0.0154

B
0.00723

C
0.00075

D
0.00035
Question 19
1 / -0

Electrolytic cell uses electrical energy to bring about

A
spontaneous chemical reactions

B
non-spontaneous chemical reactions

C
spontaneous nuclear reactions

D
non-spontaneous nuclear reactions

Solution

Electrolytic cell drives a non- spontaneous redox chemical reaction by application of electrical energy
Question 20
1 / -0

Resistivity is defined as

A
inverse of resistance

B
inverse of conductance

C
inverse of conductivity

D
inverse cell constant
Question 21
1 / -0

Standard electrode potential is measured taking the concentrations of all the species involved in a half-cell is

A
4 M

B
1 M

C
2M

D
3M

Solution

Under standard condition that is at 298K, the molar concentration of every species taken in each half cell is 1 M and if gases are involved the partial pressure of the gas is taken as 1 atm..
Question 22
1 / -0

The Nernst equation at 25°C involving the reaction Fe³+ + e^– Fe²⁺ is

A
E = E° + (RT/nF) In ([Fe²⁺]/[Fe³⁺])

B
E = E^o – (RT/nF) log ([Fe²⁺]/[Fe³⁺])

C
E = E^o – (0.0595 V) In ([Fe²⁺]/[Fe³⁺])

D
E = E^o – (0.0595 V) log ([Fe²⁺]/[Fe³⁺])
Question 23
1 / -0

The expression connecting E°_cell and K° of the reaction occurring in a galvanic cell is

A

B

C

D
Question 24
1 / -0

Given: E°(Ag⁺|Ag) = 0.799 V and E^o(Zn²⁺|Zn) = – 0.763 V. Which of the following facts is correct?

A
Ag⁺ can be reduced by H₂(g).

B
Ag can oxidise H₂(g) to H⁺.

C
Zn²⁺ can be reduced by H₂(g).

D
Ag can reduce Zn²⁺.
Question 25
1 / -0

Molar conductivity has the unit of

A

B

C

D

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