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
o
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