In the electrochemical conversion (Kolbe’s eletrolysis) of R–COONa to R–R, 1A current was passed for 965 seconds. Calculate the amount of R–R formed in this process (Faraday constant = 96,500 C mol–1)

2RCOONa+2H2O⟶2FR- Anode R+2CO2+2NaOH+H2 Cathode 1 mole of R-R = 2 F = 2 x 96500 coulombNo.of Coulombs consumed = i×t =1 x 965 =965 C No.of moles of R-R formed =9652×96500=1200 mol  ; Number of milli moles=5 ;