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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Electrolysis of dilute aqueous $NaCl$ solution was carried out by passing $10$ milliampere current. The time required to liberate $0.01 mol$ of $H_{2}$ gas at the cathode is $(1 F = 96500 C {mol}^{- 1})$

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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State Faraday's second law of electrolysis.

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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250 s

through

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solution of

M S O_{4} .

Only

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M S O_{4}

solution after electrolysis is closest to [Assume that the volume of the solution remain constant]

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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595.1

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Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

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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:

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MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

Give reason: On the basis of

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MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

Calculate the number of coulombs required to deposit

40.5 g

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when the electrode reaction is

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

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells and Electrolysis

A solution of

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5

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20

minutes. What mass of

N i

is deposited at the cathode?

Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milliampere current. The time required to liberate 0.01 mol of H2 gas at the cathode is (1 F=96500 C mol-1)

Important Questions on Electrochemistry

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Electrolysis of dilute aqueous $NaCl$ solution was carried out by passing $10$ milliampere current. The time required to liberate $0.01 mol$ of $H_{2}$ gas at the cathode is $(1 F = 96500 C {mol}^{- 1})$