Electrochemistry Test

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Electrochemistry Test - 38

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Weekly Quiz Competition

Question 1
1 / -0

Which of the following is incorrect in a galvanic cell?

A
Oxidation occurs at anode

B
Reduction occurs at cathode

C
The electrode at which electrons are gained is called cathode

D
The electrode at which electrons are lost is called cathode.

Solution

A galvanic cell is an electrochemical cell in which oxidation occurs at anode containing negative charge and reduction occurs at cathode containing a positive charge. At the anode, electrons are gained by an electrode and at the cathode, electrons are lost by an electrode.

Hence, the correct option is $$C$$
Question 2
1 / -0

Which of the following represents the oxidation half-reaction for the unbalanced redox equation?
$$Cu + HNO_{3} \rightarrow Cu (NO_{3})_{2} + NO_{2}$$

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

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

C
$$NO_{3}^{-} \rightarrow NO_{2} + 1e^{-}$$

D
$$2H^{+} + NO_{2}^{-} + 1e^{-} \rightarrow NO_{2} + H_{2}O$$

Solution

$$Cu+HNO_3 \longrightarrow Cu(NO_3)_2+NO_2$$
As Oxidation of $$Cu$$ is taking place in the reaction.
Thus the oxidation half-cell reaction will be $$Cu \longrightarrow Cu^{+2}+2e^-$$
Question 3
1 / -0

Which of the following is true for an electrolytic cell?

A
An electric current causes an otherwise nonspontanteous chemical reaction to occur.

B
Reduction occurs at the anode.

C
A spontaneous electrochemical reaction produces an electric current.

D
The electrode to which electrons flow is where oxidation occurs.

E
None of the above

Solution

For electrolytic cell following are true statements:
(a) Nonspontaneous Reduction.
(b) electrical energy $$\rightarrow $$ chemical energy
(c) Oxidation at anode ($$+ve$$ charged electrode)
Reduction at cathode ($$-ve$$ charged electrode)
Question 4
1 / -0

Examine the drawing of an electrolytic cell shown:

Determine the time it would take to plate $$10.0\ g\ Ag$$ with a current of $$0.452A$$.

A
$$2.5\ hr$$

B
$$3.5\ hr$$

C
$$4.5\ hr$$

D
$$5.5\ hr$$

Solution

we have,
$$w = \dfrac{E * I*t}{96500}$$

$$w = \dfrac{Molecular weight * I*t}{1*96500}$$

$$10 = \dfrac{108 * 0.452 * t}{96500}$$

$$t = 19768.10\, sec\, or\, 5.49 hrs$$
Question 5
1 / -0

Which of the following is the most important use of alloying?

A
Make it more beautiful

B
Gives desirable characteristics to the element

C
Provides resistance to corrosion

D
Both $$B$$ and $$C$$

Solution

Alloying is a very good method of improving the properties of a metal. It also helps in the prevention of corrosion. Thus, the correct answer is $$D$$
Question 6
1 / -0

Electrochemical equivalent is the amount of substance which gets deposited from its solution on passing electrical charge equal to :

A
$$96,500$$ coulomb

B
$$1$$ coulomb

C
$$60$$ coulomb

D
$$965$$ coulomb

Solution

Electrochemical equivalent is the amount of substance which gets deposited from its solution on passing electrical charge equal to $$96,500$$ coulomb. Note: $$96500$$ coulomb corresponds to the charge on one mole of electrons. It is called electrochemical equivalent.
Question 7
1 / -0
The breaking down of a compound by passing electricity through it is known as
A
electromagnetism

B
electrolysis

C
electronics

D
ultrasound

Solution

Electrolysis is the process of breaking down of a compound into its constituent ions by passing electricity through it.
For example : When an electric current is passed through water $$(H_2O)$$, it decomposes into $$O^{-2}$$ and $$H^+$$ ions which get further converted into Oxygen $$(O_2)$$ and Hydrogen $$H_2$$, respectively.
Question 8
1 / -0

Who invented the first true battery ?

A
Faraday

B
Ohm

C
Volta

D
Alva Edison

Solution

The first true battery was invented by the Italian physicist Alessandro Volta in 1800.

Volta stacked discs of copper (Cu) and zinc (Zn) separated by cloth soaked in salty water.

Hence, option C is correct.
Question 9
1 / -0

How many faradays are required to reduce 1 mol of $$Cr_2O_7^{2-}$$ to $$Cr^{3+}$$ in acidic medium?

A
2

B
3

C
5

D
6

Solution

$$1 \ mol\ Cr_2O_7^{2-}$$ requires 6 moles electron $$= 6F$$ charge

$$\therefore$$ Number of Faraday's required $$= 6$$.

Hence, option D is correct.
Question 10
1 / -0

What is used as anode in Volta's cell?

A
Zinc plate

B
Copper plate

C
Carbon rod

D
Iron plate

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Electrochemistry Test - 38

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Electrochemistry Test - 38

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Question 1

Oxidation occurs at anode

Reduction occurs at cathode

The electrode at which electrons are gained is called cathode

The electrode at which electrons are lost is called cathode.

Solution

Question 2

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

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

$$NO_{3}^{-} \rightarrow NO_{2} + 1e^{-}$$

$$2H^{+} + NO_{2}^{-} + 1e^{-} \rightarrow NO_{2} + H_{2}O$$

Solution

Question 3

An electric current causes an otherwise nonspontanteous chemical reaction to occur.

Reduction occurs at the anode.

A spontaneous electrochemical reaction produces an electric current.

The electrode to which electrons flow is where oxidation occurs.

None of the above

Solution

Question 4

$$2.5\ hr$$

$$3.5\ hr$$

$$4.5\ hr$$

$$5.5\ hr$$

Solution

Question 5

Make it more beautiful

Gives desirable characteristics to the element

Provides resistance to corrosion

Both $$B$$ and $$C$$

Solution

Question 6

$$96,500$$ coulomb

$$1$$ coulomb

$$60$$ coulomb

$$965$$ coulomb

Solution

Question 7

electromagnetism

electrolysis

electronics

ultrasound

Solution

Question 8

Faraday

Ohm

Volta

Alva Edison

Solution

Question 9

2

3

5

6

Solution

Question 10

Zinc plate

Copper plate

Carbon rod

Iron plate

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