Electrolytic Cells and Electrolysis

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Electrolytic Cells and Electrolysis

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Faraday's Law

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Products of Electrolysis

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Important Questions

Calculate the emf of the cell in which of the following reaction takes place:


[Given that ]

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In electrolysis of water: 

(a) Name the gas collected at cathode and anode.
(b) Why is volume of one gas collected at one electrode is double of anode?
(c) Why are few drops of dilute added to water? 

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How many electrons are there in one coulomb of electricity?

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A metal carbonate X on reacting with an acid gives a gas which when passed through a solution gives the carbonate black. On the other hand, A gas G that is obtained at anode during electrolysis of brine is passed on dry Y, it gives compound Z, used for disinfecting water. Identify X, Y, G and Z.

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How much electricity in terms of Faraday is required to produce:

(i) of from molten
(ii) of from molten

[Given : Molar mass of calcium & Aluminium are 40 g & 27 g respectively]

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How much charge is required for the following reductions?

(i) of to
(ii) of to
(iii) of to

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During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is:

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A solution of is electrolysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode?

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A solution of is electrolysed between platinum electrodes using a current of amperes for minutes. What mass of is deposited at the cathode?

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How much electricity is required in coulomb for the oxidation of:
(i) of to ?
(ii) of to ?

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