Chemistry XII - ElectroChemistry 04

Question : 1

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Correct relation is

Options:

	Electrochemical equivalent =
	One faraday = One equivalent
	One faraday = 6.023 × 1023 electrons
	All of these

Solution :

(4)

1 F = 96500 coulomb
       = 1 equivalent
       = 6 × 10²³ electrons

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Question : 2

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The total volume of gases liberated at electrodes at STP when 96.5 ampere current is passed for 10 minutes through acidified water using inert electrode is

Options:

	10.08 litre
	21.05 litre
	5.98 litre
	15.60 litre

Solution :

(1)

Total vol. of gas = 0.6 × 11.2 + 0.6 × 5.6
                             = 10.08 L

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Question : 3

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Equivalent of substance can be determined by

Options:

	Molarity × Volume litre
	All of these

Solution :

(1)

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Question : 4

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Two electrolytic cells connected in series containing aq AgNO₃ and aq. CuSO₄respectively. During electrolysis 54 g of Ag is deposited at cathode then the amount of Cu deposited would be (At. wt. of Cu = 63.5, Ag = 108)

Options:

	31.75 g
	63.5 g
	15.87 g
	45.60 g

Solution :

(3)

Eq. of Ag deposited = Eq. of Cu
deposited.

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Question : 5

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According to Faraday’s second law of electrolysis; the correct statement is

Options:

	The number of mole of substance deposited at each electrode will be equal
	The weight of the substance deposited at each electrode will be equal
	The equivalent of the substance deposited at each electrode will be equal
	The volume of each gas deposited at each electrode will be equal

Solution :

(3)

The number of equivalent of substance deposited at each electrode is same.

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Question : 6

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The number of coulombs required to deposit 4.5 g Al at cathode in the electrolysis of molten AlCl₃ using inert cathode

Options:

	48,250 C
	96,500 C
	24,125 C
	2 × 96,500 C

Solution :

(1)

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Question : 7

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Three electrolytic cells connected in series containing CuSO₄, AlCl₃ and SnCl₄ respectively in molten state. The ratio of mole of Cu : Al : Sn deposited at cathode is

Options:

	1 : 1 : 1

Solution :

(2)

n-factor of Cu, Al and Sn is 2, 3 and 4
respectively.

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Question : 8

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The number of mole of electrons required to deposit 130 g Zn is (At. wt. of Zn = 65)

Options:

	1 mole
	2 mole
	3 mole
	4 mole

Solution :

(4)

Mole of e^– = No. of eq of substance.

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Question : 9

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According to first law of electrolysis

Options:

	w = z if one faraday charge is passed
	w = z if one ampere current is passed for one minute
	w = z if one coulomb of charge is passed for one second
	w = z if one coulomb of charge is passed for one hour

Solution :

(3)

w = z if one coulomb of charge is
passed

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Question : 10

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How many faraday of charge is required to liberate 22.4 litre O₂ at STP during electrolysis of aqueous solution of CuSO₄ if the current efficiency is 25%?

Options:

	16 F
	6 F
	4 F
	8 F

Solution :

(1)

]22.4 L of O₂ = 4 eq.