Products of Electrolysis
= 3600 C We know that 96487C = 6.023 X 10 23 number of electrons .
Now , 3600 C = number of electrons . Hence ,
2.25 X 10 22 number of electrons will flow through the wire .
Problem :
Consider the reaction : Cr2 O7 2- + 14H + + 6e - → Cr 3 + + 8H2O . What is the quantity of electricity in coulombs needed to reduce 1 mol of Cr 2 O7 2- ?
Solution : Cr2 O7 2- + 14H + + 6e - → Cr 3 + + 8H2O Therefore , quantity of electricity required to reduce 1 mole of Cr 2 O7 2- = 6 F = 6 × 96487 C = 578922 C
Products of Electrolysis
o
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The product of electrolysis produced depends on the nature of material being that is being electrolyzed as well as the type of electrodes that is being used .
An inert electrode e . g ., platinum or gold does not participate in chemical reaction and acts as a source or sink for electrons .
o Whereas a reactive electrode participates in the electrode reaction . o
o
It also depends on the different oxidize in gas well as reducing species that are present in the electrolytic cell and their standard electrode potentials .
Electrolysis of molten NaCl results in the production of sodium metal and Cl2