What is electrolysis?

Electrolysis is a process that uses an electric current to break down a compound into its constituent elements.


It is often used to extract metals above carbon in the reactivity series.

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What are the main components of an electrolytic cell?'

  1. An electrolyte (an aqueous or molten ionic compound).
  2. Electrodes (cathode and anode) made from graphite or metal.
  3. A direct current supply connecting both electrodes.

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Describe the process of ion migration in an electrolytic cell.

In an electrolytic cell, positive ions (cations) migrate towards the cathode, while negative ions (anions) move towards the anode.

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At which electrodes do the processes of reduction and oxidation take place during electrolysis?

  • Reduction occurs at the cathode (the negative electrode).
  • Oxidation occurs at the anode (the positive electrode).

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What is the equation that links amount of charge transferred (Q), current (I), and time (t)?

Q = I × t


Q = charge transferred (C)

I = current (A)

t = time (s)

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What is the formula that links the Faraday constant (F), the Avogadro constant (L), and the charge of an electron (e)?

F = L × e


F = Faraday constant (C mol-1).

L = Avogadro constant (mol-1).

e = Charge of an electron (C).

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What is the Faraday constant (F)?

The Faraday constant (F) is the charge carried by one mole of electrons or one mole of singly charged ions.


Its value is approximately 96,500 C mol-1.

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What factors determine the amount of substance deposited during electrolysis?

The factors that determine the amount of substane deposited are:

  1. The size of the electric current.
  2. The time over which an electric current passes.


The larger the current and the longer the time, the greater the amount of substance deposited. 

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What factors determine the nature of the products formed at each electrode during electrolysis?

The factors that determine the products formed at each electrode are:

  1. The state of the electrolyte i.e. molten or aqueous.
  2. The relative electrode potentials of the ions present in the electrolyte.
  3. The relative concentrations of the ions present in the electrolyte.

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What substances are produced at the anode and cathode when molten magnesium bromide undergoes electrolysis?

  • Bromine is produced at the anode.
  • Magnesium is produced at the cathode.

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Explain how E⦵ values can be used to predict which cation discharges at the cathode during aqueous electrolysis.

The cation with the most positive (or least negative) E⦵ value is the easiest to reduce, so it preferentially discharges at the cathode.

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Describe the experimental procedure for determining the charge of one mole of electrons using the electrolysis of copper(II) sulfate.

  1. Separately weigh a copper anode and cathode.
  2. Arrange the apparatus as shown in the diagram above.
  3. Pass a constant electric current for a measured time interval.
  4. Remove the anode from the setup, wash, and dry.
  5. Reweigh the anode and calculate its decrease in mass.
  6. Calculate the charge of one mole of electrons using the experimental data.

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