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Thermodynamics of cell reactions | Electro Chemistry - Cell reactions | 12th Chemistry : UNIT 9 : Electro Chemistry

Chapter: 12th Chemistry : UNIT 9 : Electro Chemistry

Cell reactions

Na+ ions are attracted towards cathode, where they combine with the electrons and reduced to liquid sodium.

Cell reactions

Na+ ions are attracted towards cathode, where they combine with the electrons and reduced to liquid sodium.

Cathode (reduction)

Na+ (l ) + e- Na (l)                                Eo = -2.71V

Similarly, Cl ions are attracted towards anode where they lose their electrons and oxidised to chlorine gas.

Anode (oxidation)

2Cl- (l) Cl2 (g) + 2e-                                  Eo = -1.36V

The overall reaction is,

2Na+ (l ) + 2Cl- (l) 2Na(l ) + Cl2 (g )                        Eo = - 4.07V

The negative Eo value shows that the above reaction is a non spontaneous one. Hence, we have to supply a voltage greater than 4.07V to cause the electrolysis of molten NaCl.

In electrolytic cell, oxidation occurs at the anode and reduction occur at the cathode as in a galvanic cell, but the sign of the electrodes is the reverse i.e., in the electrolytic cell cathode is –ve and anode is +ve.

Tags : Thermodynamics of cell reactions | Electro Chemistry , 12th Chemistry : UNIT 9 : Electro Chemistry
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12th Chemistry : UNIT 9 : Electro Chemistry : Cell reactions | Thermodynamics of cell reactions | Electro Chemistry

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12th Chemistry : UNIT 9 : Electro Chemistry


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