Calculate the number of coulombs required to deposit 40 . 5 g of Al when the electrode reaction is Al 3 + + 3 e - → Al ( s ) .

Electrode reaction : Al 3 + + 3 e - → Al ( s ) Given : Weight of aluminium to be deposited = 40 . 5 g Solution : Number of electrons exchanged in 1 mol n = 3 Amount of charge deposited q = n × F Amount of charge required to deposit 1 mol of Al = 3 × 96500 Amount of charge required to deposit 1 g of Al = 3 × 96500 27 . 0 Amount of charge required to deposit 40 . 5 g of Al = 3 × 96500 × 40 . 5 27 = 434250 C Thus, 434250 coulombs are required to deposit 40 . 5 g of aluminium.

EASY

Earn 100

In an electrolytic cell, reduction occurs at .

50% studentsanswered this correctly

Important Questions on Electrochemistry

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

The anodic half-cell of lead-acid battery is recharged using electricity of

0 .05

Faraday. The amount of

{PbSO}_{4}

electrolyzed in

g

during the process is: (Molar mass of

{PbSO}_{4} = 303 g {mol}^{- 1}

)

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and 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)

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

A solution of copper sulphate electrolysed for $20$ minute with a current of $1.5$ Ampere. Calculate the mass of copper deposited at the cathode. $(F = 96500 C)$

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and 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>Electrolytic Cells and 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

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and 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>Electrolytic Cells and Electrolysis

A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes ${FeSO}_{4}$ and ${ZnSO}_{4}$ until $2.8 g$ of $Fe$ deposited at the cathode of cell X. How long did the current flow ? Calculate the mass of $Zn$ deposited at the cathode of cell Y.

$($ Molar mass : $Fe = 56 g {mol}^{- 1} Zn = 65.3 g {mol}^{- 1}, 1 F = 96500 C {mol}^{- 1}$ $)$

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and 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>Electrolytic Cells and Electrolysis

State Faraday's first law of electrolysis.

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

State Faraday's second law of electrolysis.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and 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>Electrolytic Cells and 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>Electrolytic Cells and 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>Electrolytic Cells and Electrolysis

What are galvanic cells? Explain the working of a galvanic cell with a neat sketch taking Daniel cell as example.

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and 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>Electrolytic Cells and Electrolysis

The weight of silver (at.wt.

= 108

) displaced by a quantity of electricity which displaces

5600 m L

O_{2}

STP

will be

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

108 g

of silver (molar mass

108 g {m o l}^{- 1}

) is deposited at cathode from

{A g N O}_{3} (a q)

solution by a certain quantity of electricity. The volume (in

L

) of oxygen gas produced at

273 K

and

1

bar pressure from water by the same quantity of electricity is

\frac{x}{10}

. Value of

' x'

to the nearest integer is _____.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

Give reason: On the basis of

E^{\circ}

values,

O_{2}

gas should be liberated at anode but it is

{Cl}_{2}

gas which is liberated during electrolysis of aqueous

NaCl

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

Calculate the number of coulombs required to deposit

40.5 g

Al

when the electrode reaction is

{Al}^{3 +} + 3 e^{-} \to Al (s)

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

A solution of

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

is electrolyzed between platinum electrodes using a current of

5

amperes for

20

minutes. What mass of

N i

is deposited at the cathode?

In an electrolytic cell, reduction occurs at .

Important Questions on Electrochemistry

Learn and Prepare for any exam you want !