Electrochemistry Test

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Electrochemistry Test - 17

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Weekly Quiz Competition

Question 1
1 / -0

What should be the state of compounds which decompose on passing electric current?

A
Plasma

B
Solid

C
Gas

D
Molten or aqueous

Solution

Compounds should be aqueous or molten so that they can be easily dissociated into ions.
Question 2
1 / -0

Anode is

A
positively charged electrode

B
negatively charged electrode

C
wire used to connect the electrodes

D
electrolyte which conducts electricity

Solution

An Anode is a positively charged electrode through which conventional current flows in a circuit .
Question 3
1 / -0

Electrolytes which allow small amount of electricity to pass through them are known as :

A
strong electrolytes.

B
weak electrolytes.

C
non-electrolytes.

D
none of the above.

Solution

Electrolytes which allow small amount of electricity to pass through them are known as weak electrolytes.

Hence, the correct option is $$B$$.
Question 4
1 / -0

Carbon dioxide is a __________.

A
weak electrophile

B
weak nucleophile

C
ambident species

D
none of these

Solution

Carbon dioxide is a weak electrophile. It possess very less partial positive charge which are attracted towards electrons.
Question 5
1 / -0

The process in which chemical change occurs on passing electricity is termed as __________.

A
ionisation

B
neutralisation

C
electrolysis

D
hydrolysis

Solution

Electrolysis is a process by which electric current is passed through a substance to effect a chemical change i.e oxidation or reduction of a substance.
Question 6
1 / -0

A Faraday is:

A
the magnitude of the charge of $$1\ mole$$ of electrons

B
the magnitude of the electric dipole

C
a fundamental constant of nature equal to $$6.63 \times 10^{-34}Js/photon$$

D
a constant that accounts for the existence of ions in solution

Solution

Option A is the correct answer.
One Faraday is defined as the amount of charge carried by $$1$$ mole of electrons.
Question 7
1 / -0

Which of the following condition is correct for operation of electrolytic cell?

A
$$\triangle G = 0, E = 0$$

B
$$\triangle G < 0, E > 0$$

C
$$\triangle G > 0, E < 0$$

D
$$\triangle G > 0, E > 0$$

Solution

Electrolytic cell is an electrochemical cell that drives a non-spontaneous reaction,
that means $$\Delta G >0\ and\ E <0$$
Question 8
1 / -0

Consider the given circuit carefully, What do you think would happen if the two copper plates are moved further apart from each other ?

A
Larger amount of copper will be deposited on the plate connected to the negative electrode

B
Smaller amount of copper will be deposited on the plate connected to the negative electrode

C
Larger amount of copper will be deposited on the plate connected to the positive electrode

D
Smaller amount of copper will be deposited on the plate connected to the positive electrode

Solution

Reduction at cathode (negative electrode) : $$Cu^{+2} + 2e^{-1}_0 \rightarrow Cu$$
$$Cu^{+2}$$ ions from the solution gets attracted by the negative electrode (cathode) which have excess electrons. These $$Cu^{+2}$$ ions take the electrons from the cathode and thus gets reduced as $$Cu$$ atoms. As the two copper plates are moved further, more and more $$Cu^{+2}$$ ions are reduced at the cathode and hence larger amount of copper deposits on the plate connected plates to the negative electrode (cathode).
Question 9
1 / -0

$$Zn(s)|ZnCl_2(aq)| |Cl^-(aq)|Cl_2(g)|C(s)$$
In the electrochemical cell described by the cell diagram above, what reaction occurs at the anode?

A
$$Zn \rightarrow Zn^{2+}+2e^-$$

B
$$Zn^{2+}+2e^- \rightarrow Zn$$

C
$$Cl_2 + 2e^-\rightarrow 2Cl^-$$

D
$$2Cl^- \rightarrow Cl_2 +2e^-$$

Solution

In the given cell diagram, the reaction taking place at the anode is
$$Zn \rightarrow Zn^{2+} + 2e^-$$ at the anode, oxidation of zinc takes place.
Question 10
1 / -0

Statement 1: In an electrochemical cell, the electrode that is the site of reduction is called the anode.
Statement 2: Oxidation always occurs at the cathode.

A
Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

B
Both the Statement 1 and Statement 2 are correct, but Statement 2 is NOT the correct explanation of Statement 1.

C
Statement 1 is correct, but Statement 2 is not correct.

D
Both the Statement 1 and Statement 2 are not correct.

Solution

both are incurrect because
in an electrochemical cell the electrode that is the site of reduction is called the cathode and the oxidation always occurs at the anode
so the both statement are incurrect

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Electrochemistry Test - 17

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Electrochemistry Test - 17

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Question 1

Plasma

Solid

Gas

Molten or aqueous

Solution

Question 2

positively charged electrode

negatively charged electrode

wire used to connect the electrodes

electrolyte which conducts electricity

Solution

Question 3

strong electrolytes.

weak electrolytes.

non-electrolytes.

none of the above.

Solution

Question 4

weak electrophile

weak nucleophile

ambident species

none of these

Solution

Question 5

ionisation

neutralisation

electrolysis

hydrolysis

Solution

Question 6

the magnitude of the charge of $$1\ mole$$ of electrons

the magnitude of the electric dipole

a fundamental constant of nature equal to $$6.63 \times 10^{-34}Js/photon$$

a constant that accounts for the existence of ions in solution

Solution

Question 7

$$\triangle G = 0, E = 0$$

$$\triangle G < 0, E > 0$$

$$\triangle G > 0, E < 0$$

$$\triangle G > 0, E > 0$$

Solution

Question 8

Larger amount of copper will be deposited on the plate connected to the negative electrode

Smaller amount of copper will be deposited on the plate connected to the negative electrode

Larger amount of copper will be deposited on the plate connected to the positive electrode

Smaller amount of copper will be deposited on the plate connected to the positive electrode

Solution

Question 9

$$Zn \rightarrow Zn^{2+}+2e^-$$

$$Zn^{2+}+2e^- \rightarrow Zn$$

$$Cl_2 + 2e^-\rightarrow 2Cl^-$$

$$2Cl^- \rightarrow Cl_2 +2e^-$$

Solution

Question 10

Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

Both the Statement 1 and Statement 2 are correct, but Statement 2 is NOT the correct explanation of Statement 1.

Statement 1 is correct, but Statement 2 is not correct.

Both the Statement 1 and Statement 2 are not correct.

Solution

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