Electrochemistry Test

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Electrochemistry Test - 54

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Weekly Quiz Competition

Question 1
1 / -0

In electrolysis, if the duration of the passage of current is doubled, the mass liberated is

A
Doubled

B
Halved

C
Increased

D
Remains the same

Solution

According to Faraday’s First Law of Electrolysis, mass of the substance (m) deposited or liberated at any electrode is directly proportional to the quantity of electricity or charge (Q) passed.
m = Z x I x t ; (I = Q/t)
where m is the mass of the substance produced in g; Z is the electrochemical equivalent, which is the mass of a substance produced at the electrode during electrolysis by one coulomb of charge
Z=(atomic weight/ nF)
I is the current in Ampere(A); t is the time in seconds;
Hence if the duration of the passage of current (t) is doubled then,
m’ = Z x I x (2t) = 2 (Z x I x t) = 2m

So, the mass liberated (m) will also be doubled. [Option A]
Question 2
1 / -0

To deposit one gm equivalent of an element at an electrode, the quantity of electricity needed is

A
One ampere

B
$$96000 $$ amperes

C
$$96500 $$ farads

D
$$96500$$ coulombs

Solution

$$96500$$ coulombs of charge is needed to deposit one gram equivalent of an element at an electrode.
Question 3
1 / -0

E.C.E. of Cu and Ag are$$7\times 10^{-6}$$ and $$1.2\times 10^{-6}$$ certain current deposits 14 gm of Cu. Amount of Ag deposited is

A
1.2 gm

B
1.6 gm

C
2.4 gm

D
1.8 gm

Solution

mass deposit $$m\propto ECE$$
so $$\dfrac{m_1}{m_2}=\dfrac{E_1}{E_2}$$

$$\dfrac{14}{m_2}=\dfrac{7\times 10^{-6}}{1.2\times 10^{-6}}$$

$$m_2=2.4\,gm$$
Hence Amount of Ag deposited is 1.2 gm
Question 4
1 / -0

In the process of electrolysis, the current is carried out inside the electrolyte by

A
Electrons

B
Atoms

C
Positive and negative ions

D
All the above

Solution

Electrolyte Solution or molten salt can conduct electricity by the process of electrolysis. In electrolytes, current is carried by positive and negative ions, rather than by electrons.
For example, in a lead-acid car battery, the electrolyte is dilute sulphuric acid, which contains negative sulphate ions and positive hydrogen ions. [Option C]
Question 5
1 / -0

The compound $$75$$ decomposed into its constituents under the effect of electric current is called:

A
Electrolysis

B
Hydrolysis

C
Electroplating

D
Corrosion

Solution
Question 6
1 / -0

The chemical equivalent of copper and zinc are 32 and 108 respectively. When copper and silver voltameter are connected in series and electric current is passed through for sometimes, 1.6 g of copper is deposited. Then, the mass of silver deposited will be

A
3.5 g

B
2.8 g

C
5.4 g

D
None of these

Solution

From Faraday’s law, m/E = constant
where m = mass of substance deposited, E =chemical equivalent. $$ \therefore \dfrac{m_{2}}{m_{1}} = \dfrac{E_{2}}{E_{1}} \Rightarrow m_{2} = \dfrac{108}{32} \times 1.6 = 5.4g $$
Question 7
1 / -0

What makes the electric current flow through electric solution ?

A
Only free electrons

B
Only positive ions.

C
Only negative ions

D
Positive and negative ions

Solution

Electric current flows through electric solution by means of $$\textbf{positive and negative ions}$$
Question 8
1 / -0

If a half cell reaction, $$ A+e^{-} \longrightarrow A^{-} $$ has a large negative reduction potential, it follows that

A
$$ \mathrm{A} $$ is easily reduced

B
$$A $$ is readily oxidized

C
$$ \mathrm{A}^{-} $$ is readily reduced

D
$$ \mathrm{A}^{-} $$ is readily oxidised.

Solution

$$\text{Large negative potential for the reaction, } A + e ^ { - } \rightarrow \mathrm{A}^{-} $$ implies that the reverse reaction occurs,i.e., $$ A^{-} $$ is readily oxidised.
Question 9
1 / -0

In a galvanic cell, the electrons flow from

A
anode to the cathode through the solution

B
cathode to the anode through the solution

C
anode to the cathode through the external circuit

D
cathode to the anode through the external circuit

Solution

anode to the cathode through the external circuit
Question 10
1 / -0

In Nickel-Silver nitrate cell, silver acts as a :

A
cathode

B
anode

C
salt bridge

D
none of these

Solution

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Electrochemistry Test - 54

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Electrochemistry Test - 54

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Question 1

Doubled

Halved

Increased

Remains the same

Solution

Question 2

One ampere

$$96000 $$ amperes

$$96500 $$ farads

$$96500$$ coulombs

Solution

Question 3

1.2 gm

1.6 gm

2.4 gm

1.8 gm

Solution

Question 4

Electrons

Atoms

Positive and negative ions

All the above

Solution

Question 5

Electrolysis

Hydrolysis

Electroplating

Corrosion

Solution

Question 6

3.5 g

2.8 g

5.4 g

None of these

Solution

Question 7

Only free electrons

Only positive ions.

Only negative ions

Positive and negative ions

Solution

Question 8

$$ \mathrm{A} $$ is easily reduced

$$A $$ is readily oxidized

$$ \mathrm{A}^{-} $$ is readily reduced

$$ \mathrm{A}^{-} $$ is readily oxidised.

Solution

Question 9

anode to the cathode through the solution

cathode to the anode through the solution

anode to the cathode through the external circuit

cathode to the anode through the external circuit

Solution

Question 10

cathode

anode

salt bridge

none of these

Solution

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