The weight in grams of O₂ formed at Pt anode during the electrolysis of aq. ${\mathrm{K}}_2{\mathrm{SO}}_4$ solution during the passage of one coulomb of electricity is 

When K₂SO_{4 (aq)} is electeolysed the product formed at anode is O₂ and at cathode is H₂ . 

According to Faraday's law of electrolyis , 

w= zQ 

w= mass of substance .

Q= charge .

z= electrochemical equivalent .

Electrochemical equivalent (z)is defined as the mass of substnace deposited when one coulomb of electricity is passed through the electrolyte. 

$z= \frac{Equivalent weight }{96500}$

Hence the mass of oxygen O formed when one coulomb of elceticity passed = $\frac{Equivalent weight of O_{2 }}{96500}=\frac{8}{96500}$g