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An aqueous solution of $0.02 M {MgSO}_{4}$ electrolysed by passing a current of $9.65 A$ for $30 \min$ . Mass of product obtained at cathode is

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Important Questions on Electrochemistry

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Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

One litre solution of

{MgCl}_{2}

is electrolyzed completely by passing a current of

1 A

for

16 \min 5

sec. The original concentration of

{MgCl}_{2}

solution was (Atomic mass of

Mg = 24

)

EASY

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

A solution of

N i {(N O_{3})}_{2}

is electrolyzed between platinum electrode

0.1

Faraday electricity. How many mole of

N i

will be deposited at the cathode?

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

When

0.1 m o l {M n O}_{4}^{2 -}

is oxidized the quantity of electricity required to completely

M n O_{4}^{2 -}

M n O_{4}^{-}

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Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

0.5 F

of electricity is passed through

500 mL

of copper sulphate solution. The amount of copper which can be deposited will be

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

When 9.65 ampere current was passed for 1.0 hour into nitrobenzene in acidic medium, the amount of p-aminophenol produced is:

EASY

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

The quantity of electricity needed to separately electrolyse

1 M

solution of

{ZnSO}_{4}, {AlCl}_{3}

and

{AgNO}_{3}

completely is in the ratio of

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

The weight of silver (at.wt.

= 108

) displaced by a quantity of electricity which displaces

5600 m L

O_{2}

STP

will be

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

For the oxidation of

0.2 M {FeSO}_{4}

solution

0.965

amperes current is passed through it for

1

hour. The volume of the solution that is oxidised in

mL

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

A current of $10.0 A$ flows for $2.00 h$ through an electrolytic cell containing a molten salt of metal $X$ . This results in the decomposition of $0.250 mol$ of metal $X$ at the cathode. The oxidation state of $X$ in the molten salt is:

$(F = 96, 500 C)$

HARD

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

How long (approximate) should water be electrolysed by passing through

100

amperes

current so that the oxygen released can completely burn

27.66 g

of diborane? (Atomic weight of

B = 10.8 u

)

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

What time in sec is required for depositing all the silver present in

125 ml

1 M {AgNO}_{3}

solution by passing a current of

241.25

A (Given

1 F = 96500 C

)

EASY

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

During the electrolysis of molten sodium chloride, the time required to produce

0.10 mol

of chlorine gas using a current of

3 amperes

HARD

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

0.804 A

current is passed through an aqueous solution of

NaCl

for

10

minutes. The volume of

0.05 N H_{2} {SO}_{4}

needed to neutralize the base is

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

The number of Faradays(F) required to produce

20 g

of calcium from molten

{CaCl}_{2}

(Atomic mass of

Ca = 40 g {mol}^{- 1}

) is

HARD

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

Consider the electrochemical reaction between

Ag (s)

and

{Cl}_{2} (g)

electrodes in

1 litre

0.1 M KCl

aqueous solution. Solubility product of

AgCl

1.8 \times 10^{- 10}

and

F = 96500 C {mol}^{- 1}

When a current of

10 μ A

is passed, calculate the minimum time in seconds(

s

) required to observe the

AgCl

precipitation in the galvanic cell.

EASY

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

What amount of electricity can deposit

1

mole of Al metal at cathode when passed through molten

{AlCl}_{3}

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Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

{CuSO}_{4}

solution is electrolysed for

15

minutes to deposit

0.4725 g

of copper at the cathode. The current in amperes required is

(

Faraday

= 96, 500 {Cmol}^{- 1}

, atomic weight of copper

= 63)

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

Oxidation of succinate ion produces ethylene and carbon dioxide gases. On passing

0.2

Faraday electricity through an aqueous solution of potassium succinate, what is the total volume of gases (at both cathode and anode) at STP (

1 atm

and

273 K

EASY

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

The number of electrons delivered at the cathode, during electrolysis by a current of

1 ampere in 60 seconds

is (charge on electron

= 1.60 \times 10^{- 19} C

)

EASY

Chemistry>Physical Chemistry>Electrochemistry>Faraday’s Laws of Electrolysis

Two Faraday of electricity is passed through a solution of

C u S O_{4}

. The mass of copper deposited at the cathode is: (Atomic mass of Cu = 63.5 amu)

An aqueous solution of 0.02M MgSO4 electrolysed by passing a current of 9.65A for 30min. Mass of product obtained at cathode is

Important Questions on Electrochemistry

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An aqueous solution of $0.02 M {MgSO}_{4}$ electrolysed by passing a current of $9.65 A$ for $30 \min$ . Mass of product obtained at cathode is