Electrochemistry Test

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Electrochemistry Test - 72

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Weekly Quiz Competition

Question 1
1 / -0

In the galvanic cell, $$Cu|{ Cu }^{ 2+ }(1M)\parallel { Ag }^{ + }(1M)|Ag$$, the electrons will travel in the external circuit:

A
from $$Ag$$ to $$Cu$$

B
from $$Cu$$ to $$Ag$$

C
electrons do not travel in the external circuit

D
none of these

Solution
Question 2
1 / -0

$${ E }_{ cell }^{ o }$$ for the reaction $$Co(s)+{ Ni }^{ 2+ }\quad \longrightarrow { Co }^{ 2+ }+Ni(s)$$ is $$+0.03$$ volt. If cobalt metal is added to an aqueous solution having $$\left[ { Ni }^{ 2+ } \right] =1M$$

A
the reaction will not proceed in the forward direction at all

B
the displacement of $${Ni}^{2+}$$ from solution by $$Co$$ will go to completion

C
the displacement of $${Ni}^{2+}$$ from solution by $$Co$$ will proceed to a considerable extent, but the reaction will stop before the $${Ni}^{2+}$$ is completely displaced

D
only the reverse reaction will occur

Solution
Question 3
1 / -0

Directions For Questions

The process of corrosion of iron is known as rusting. Rust appears to be a hydrated ferric oxide, $$Fe_{2}O_{3}\cdot xH_{2}O.$$ Both $$O_{2}$$ and $$H_{2}O$$ are required of rusting. Iron can be protected from rusting by use of the following methods:
(i) Applying paints, lacquers, and enamels on the surface of the iron.
(ii) By forming a firm and coherent protective coating of ferrosoferric oxide. This is done by passing steam over a hot iron.
(iii) By coating a thin film of zinc, tin, nickel, chromium, aluminum, etc., on the surface of the iron.
If plated with zinc, the reaction products of zinc with $$O_{2}$$ and $$H_{2}O$$ from a coating which sticks to the surface and thereby protects iron.

...view full instructions

Corrosion is an electrochemical process. It involves:

A
Loss of electrons by iron, $$Fe\longrightarrow Fe^{2+}+2e$$. i.e iron acts as an anode

B
Impurities act as a cathode. Electrons are used in forming hydroxyl ions
$$H_2O+O+2e \longrightarrow 2OH^-$$

C
Ferrous ions are oxidised to ferries ions in presence of dissolved oxygen.
$$2Fe^{2+}+O+H_2O\longrightarrow 2Fe^{3+}+2OH^-$$

D
All the above reactions

Solution

Question 4

1 / -0

The standard reduction potential data at $${25}^{o}C$$ is given below:

(i) $${ E }^{ o }\left( { Fe }^{ 3+ },{ Fe }^{ 2+ } \right) =-0.77V$$
(ii) $${ E }^{ o }\left( { Fe }^{ 2+ },{ Fe }^{ } \right) =-0.44V$$
(iii) $${ E }^{ o }\left( { Cu }^{ 2+ },{ Cu }^{ } \right) =+0.34V\quad $$
(iv) $${ E }^{ o }\left( { Cu }^{ + },{ Cu }^{ } \right) =+0.52V$$
(v) $${ E }^{ o }({ O }_{ 2\ (g)}+{ H }^{ + }+4e\rightarrow 4O{ H }^{ - })=+1.23V$$
(vi) $${ E }^{ o }({ O }_{ 2\ (g)}+2{ H }_{ 2 }O+4e\rightarrow 4{ OH }^{ - })=+0.40V$$
(vii) $${ E }^{ o }\left( { Cr }^{ 3+ },{ Cr }^{ } \right) =-0.74V$$
(viii) $${ E }^{ o }\left( { Cr }^{ 2+ },{ Cr }^{ } \right) =+0.91V\quad $$

Match $${E}^{o}$$ of the redox pair in List-I with the values given in List-II and select the correct answer using the code given below the lists

List I	List II
(P) $${E}^{o}({ Fe }^{ 3+ },{ Fe })$$	(1) $$-0.18V$$
(Q) $${E}^{o}(4{ H }_{ 2 }O\rightleftharpoons 4{ H }^{ + }+4{ OH }^{ - })$$	(2) $$-0.4V$$
(R) $${E}^{o}({ Cu }^{ + },{ Cu }\rightarrow 2{Cu}^{+})$$	(3) $$-0.04V$$
(S) $${E}^{o}({Cr}^{3+},{Cr}^{2+})$$	(4) $$-0.83V$$

$$P-4; Q- 1; R-2; S-3$$

$$P-2; Q- 3; R-4; S-1$$

$$P-1; Q- 2; R-3; S-4$$

$$P-3; Q- 4; R-1; S-2$$

Solution

Question 5
1 / -0

$$\cfrac { 1 }{ 2 } { H }_{ 2 }(g)+AgCl(s)={ H }^{ + }(aq)+{ Cl }^{ - }(aq)+Ag(s)$$ occurs in the galvanic cell:

A
$$Ag/AgCl(s)|KCl(sol)\parallel Ag{ NO }_{ 3 }(sol)|Ag\quad $$

B
$$Pt/{ H }_{ 2 }(g)|HCl(sol)\parallel Ag{ NO }_{ 3 }(sol)|Ag$$

C
$$Pt/{ H }_{ 2 }(g)|HCl(sol)\parallel AgCl(s)|Ag$$

D
$$Pt/{ H }_{ 2 }(g)|KCl(sol)\parallel AgCl(s)|Ag$$

Solution

$$\cfrac { 1 }{ 2 } { H }_{ 2 }(g)+AgCl(s)={ H }^{ + }(aq)+{ Cl }^{ - }(aq)+Ag(s)$$

$$Pt/{ H }_{ 2 }(g),HCl(sol)\parallel AgCl(s)/{ Ag }^{ 2+ }$$

Hence, option C is correct.
Question 6
1 / -0

One coulomb is the charge of

A
$$1$$ mole of electrons

B
$$\dfrac{1}{96500}$$ mole of electrons

C
$$\% 500$$ moles of electrons

D
$$none\ of\ these$$

Solution
Question 7
1 / -0

Unit of Faraday is

A
Ampere

B
Coulomb

C
Coulomb $$mole^{-1}$$

D
Coulomb $$sec^{-1}$$

Solution

In the International System of Units ( SI ), the coulomb (C) is the preferred unit of electric charge quantity. It is equivalent to one ampere-second (1 A.s) and represents approximately $$6.24 * 10^{ 18}$$ electric charge carriers. To convert from coulombs to faradays, multiply by $$1.04 *10^{ -5}$$ .
Question 8
1 / -0

Which of the following facts about the chemical cell and concentration cell is correct?

A
Chemical cell is an electrolytic cell whereas concentration cell is a galvanic cell

B
Chemical cell has an overall cell reaction whereas the concentration cell has no overall reaction.

C
Two half cells of both the chemical and concentration cells are chemically different

D
$${E}_{cell}$$ equations (Nernst equation) of both the cells have the therm $${E}_{cell}^{o}$$

Solution
Question 9
1 / -0

When one of ampere current flows for $$1\ sec$$ through a conductor, this quantity of electricity is known as

A
Faraday

B
Coulomb

C
E.M.F

D
Ohm

Solution

$$\text{When one of ampere current flows for 1 sec through a conductor, this quantity of electricity is known as E.M.F.}$$.
therefore option (C) is a correct answer.
Question 10
1 / -0

Hydrogen-oxygen fuel cells are used in space-craft to supply:

A
Illumination

B
Hydrogen

C
Oxygen

D
Water

Solution

Fuel-cells are used to provide power and drinking water to astronauts in space programme.

Option D is correct.

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Electrochemistry Test - 72

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Electrochemistry Test - 72

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Question 1

from $$Ag$$ to $$Cu$$

from $$Cu$$ to $$Ag$$

electrons do not travel in the external circuit

none of these

Solution

Question 2

the reaction will not proceed in the forward direction at all

the displacement of $${Ni}^{2+}$$ from solution by $$Co$$ will go to completion

the displacement of $${Ni}^{2+}$$ from solution by $$Co$$ will proceed to a considerable extent, but the reaction will stop before the $${Ni}^{2+}$$ is completely displaced

only the reverse reaction will occur

Solution

Question 3

Loss of electrons by iron, $$Fe\longrightarrow Fe^{2+}+2e$$. i.e iron acts as an anode

Impurities act as a cathode. Electrons are used in forming hydroxyl ions$$H_2O+O+2e \longrightarrow 2OH^-$$

Ferrous ions are oxidised to ferries ions in presence of dissolved oxygen.$$2Fe^{2+}+O+H_2O\longrightarrow 2Fe^{3+}+2OH^-$$

All the above reactions

Solution

Question 4

$$P-4; Q- 1; R-2; S-3$$

$$P-2; Q- 3; R-4; S-1$$

$$P-1; Q- 2; R-3; S-4$$

$$P-3; Q- 4; R-1; S-2$$

Solution

Question 5

$$Ag/AgCl(s)|KCl(sol)\parallel Ag{ NO }_{ 3 }(sol)|Ag\quad $$

$$Pt/{ H }_{ 2 }(g)|HCl(sol)\parallel Ag{ NO }_{ 3 }(sol)|Ag$$

$$Pt/{ H }_{ 2 }(g)|HCl(sol)\parallel AgCl(s)|Ag$$

$$Pt/{ H }_{ 2 }(g)|KCl(sol)\parallel AgCl(s)|Ag$$

Solution

Question 6

$$1$$ mole of electrons

$$\dfrac{1}{96500}$$ mole of electrons

$$\% 500$$ moles of electrons

$$none\ of\ these$$

Solution

Question 7

Ampere

Coulomb

Coulomb $$mole^{-1}$$

Coulomb $$sec^{-1}$$

Solution

Question 8

Chemical cell is an electrolytic cell whereas concentration cell is a galvanic cell

Chemical cell has an overall cell reaction whereas the concentration cell has no overall reaction.

Two half cells of both the chemical and concentration cells are chemically different

$${E}_{cell}$$ equations (Nernst equation) of both the cells have the therm $${E}_{cell}^{o}$$

Solution

Question 9

Faraday

Coulomb

E.M.F

Ohm

Solution

Question 10

Illumination

Hydrogen

Oxygen

Water

Solution

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Impurities act as a cathode. Electrons are used in forming hydroxyl ions
$$H_2O+O+2e \longrightarrow 2OH^-$$

Ferrous ions are oxidised to ferries ions in presence of dissolved oxygen.
$$2Fe^{2+}+O+H_2O\longrightarrow 2Fe^{3+}+2OH^-$$