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.

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Explain electrolysis of aqueous solution of ${CuBr}_{2}$ gives $Cu$ at the cathode and ${Br}_{2}$ at the anode.

Important Questions on Electrochemistry

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

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}

)

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

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

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. $(F = 96500 C)$

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

During the electrolysis of aqueous sodium chloride, the product obtained at anode is

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

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

If an aqueous solution of

NaF

is electrolyzed between inert electrodes, the product obtained at anode is

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

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

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

The $pH$ of the solution _________ during the electrolysis of dilute aqueous solution of ${CuSO}_{4} .$

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

State Faraday's first law of electrolysis.

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

State Faraday's second law of electrolysis.

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

In the preparation of chlorine by the electrolysis of brine, the reaction taking place at the anode is

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

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?

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

If electrolysis of aqueous

{CuSO}_{4}

solution is carried out using

Cu

-electrodes, the reaction taking place at the anode is

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

An aqueous solution of

{CuSO}_{4}

is subjected to electrolysis using inert electrodes. The

pH

of the solution will

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

Electrolysis of concentrated aqueous solution of

NaCl

results in

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

Electric current was passed through an aqueous solution of

{CuSO}_{4}

using two

Pt

electrodes. After some time, the blue colour of the solution disappeared along with evolution of

O_{2}

gas. Which of the following statement is correct regarding the resultant solution?

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

When electricity is passed through a solution of

{AlCl}_{2}

13.5 g

Al

is deposited at the cathode. The number of faradays passed is

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

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

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

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

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?

Explain electrolysis of aqueous solution of CuBr2 gives Cu at the cathode and Br2 at the anode.

Important Questions on Electrochemistry

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Explain electrolysis of aqueous solution of ${CuBr}_{2}$ gives $Cu$ at the cathode and ${Br}_{2}$ at the anode.