Question
Calculate the number of coulombs required for the oxidation of 1 mole of water to oxygen as per equation:
2H2O → 4H+ + O2 + 4e–
[Given: 1 F = 96,500 C mol–1]
Solution
2H2O → 4H+ + O2 + 4e–
Formula required charge n × F
n = difference of charge on ions
F is constant and equal to 96500 Coulombs
Here n = 2
2 moles of H2O require 4 x 96500 C
1 mole of H2O will need
