The process of using an electric current to bring about chemical change is called electrolysis.Electrolysis is a processes of oxidation and reduction at the respective electrodes due to external current passed in the electrolyte. The product obtained during electrolysis depends on following factors. The nature of the electrolyte The concentration of electrolyte The nature of the electrode. Consider the electrolysis of following cell containing aq. solution of `CuSO_4,ZnCl_2` and `MBr_2` by using pure silver rod as a cathode and Pt electrode as anode.Assume that `M^(2+)` does not further oxidise and can not form complex with `NH_3` Assume no hydrolysis of any ion. `E_(Cu^(2+)//Cu)^(0)=0.35 V, E_(M^(2+)//M)^(0)=-0.10 V, E_(Zn^(2+)//Zn)^(0)=-0.76 V, E_(H_(2)O // H_2)^(0)=-0.828 V, E_(Ag^(+)//Ag)^(0)=0.80 V, (2.303RT)/F=0.06` What will be the volume of gases formed at anode at STP by electrolysis of above solution after passing 20 amp current for 28950 sec. (Assume current efficiency to be 100% and one mole of gas occupies 22.4 L volume at STP). A. `44.8 L Br_2`B. `22.4 L Br_2`C. `22.4 L Cl_2`D. `44.8 L Cl_2`