Electrolytic cell and electroplating
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Electrolytic Cell and Electroplating. Chapter 19 Page 776-781 Chem 12. An electrolytic cell is a device in which an external source of electrons (electrical circuit) is used to make a non-spontaneous redox reaction take place.

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Electrolytic Cell and Electroplating

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Electrolytic cell and electroplating

Electrolytic Cell and Electroplating

Chapter 19 Page 776-781

Chem 12


Electrolytic cell and electroplating

  • An electrolytic cellis a device in which an external source of electrons (electrical circuit) is used to make a non-spontaneous redox reaction take place.

  • Molten (liquid) state of a pure substance is the medium which the cell is made. Ex: molten NaCl


Electrolytic cell and electroplating

  • Oxidation at anode

    2Cl- Cl2 + 2e-

  • Reduction at cathode

    Na+ + 1e- Na


Electrolytic cell and electroplating

NOTE:

The cathode is still under going reduction, but now is negative.

The anode is still under going oxidation, but now is positive.

REASON:

  • The electrodes are connected to a power source that pump e- from negative to positive.

  • The electrode that is connected to the power source is the cathode.

  • Since electrons are being forced into the cathode it becomes negative.


Electrolytic cell and electroplating

  • An example of an electrolytic cell is when molten NaCl is electrolyzed to form liquid sodium and chlorine gas. The sodium ions migrate toward the cathode, where they are reduced to sodium metal. Similarly, chloride ions migrate to the anode and are oxided to form chlorine gas.


Electrolytic cell and electroplating

  • E0net= E0ox + E0red

    = (-1.36 V) + (-2.71 V)

    = -4.07 V

  • The net cell voltage of -4.07

  • Because it is a non-spontaneous reaction the E0net is always less than zero.


Electrolytic cell and electroplating

  • In the electrolytic cells using molten ionic compounds, the negative ions will be oxidized.

  • The two electrodes used in an electrolytic cell do not take part in any reaction. They are non-reactive. Ex: carbon and platinum.


Electroplating

Electroplating


Electrolytic cell and electroplating

  • Electroplatingis a procedure that uses electrolysis to apply a thin layer of a metal over the surface of another metal.

  • Electrolysisis the process of making a non-spontaneous chemical redox reaction occur by passing electricity through a substance. (electrolytic cell)


Electrolytic cell and electroplating

  • In electroplating, the anode is made up of the metal you want to coat the surface of another metal with.

  • There is also a salt solution present of the anode metal.

  • While electrolysis is taking place, the anode metal is oxidized and goes into solution as positive ions.

  • These positive ions are then reduced on the surface of the cathode (the metal you wish to coat).


Examples of electroplating

Examples of electroplating

  • Coating jewlery with thin layer of expensive metal.

  • Coating chromium over steel to make rust resistant.


Sample problem 1

SAMPLE PROBLEM 1

A spoon is to be plated with silver, Ag.

  • Identify the anode and cathode.

  • Write an equation for the reaction taking place at the anode and at the cathode and indicate whether it is oxidation or reduction.

  • What electrolyte is used?


Answer

ANSWER

1. Cathode = spoon (metal object to be coated), Anode = silver electrode

2. As electrolysis takes place, the silver anode is oxidized,

Ag(s) → Ag+(aq) + 1e-

  • The Ag+ (aq) ions in solution travel to the spoon cathode and are reduced to form neutral Ag(s) on the surface of the spoon (cathode):

    Ag+ (aq) + 1e- → Ag(s)


Electrolytic cell and electroplating

3. Electrolyte solution is made of AgNO3


Sample problem 2

SAMPLE PROBLEM 2

A knife to be used as an eating utensil is to be plated with gold, Au.

a) Sketch and label a diagram of the apparatus used to electroplate the knife with gold.

b) Identify the anode and cathode.

c) Write an equation for the reaction taking place at the anode and at the cathode and indicate whether it is oxidation or reduction.

d) What electrolyte is used?


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