(a). Two electrolytic cells containing silver nitrate solution and dilute sulphuric acid solution were connected in series. A steady current of 2.5 amp was passed through them till 1.078g of silver was deposited (Ag=107.8" g "mol^(-1),1F=96500C] (i) How much electricity was consumed? (ii) What was the weight of oxygen gas liberated?

(a). Two electrolytic cells containing silver nitrate solution and dil

1.	(a). Two electrolytic cells containing silver nitrate solution and dilute sulphuric acid solution were connected in series. A steady current of 2.5 amp was passed through them till 1.078g of silver was deposited (Ag=107.8" g "mol^(-1),1F=96500C] (i) How much electricity was consumed? (ii) What was the weight of oxygen gas liberated?
Answer» Solution :(i) `Ag^(+)+etoAg, 1 mol (107.8g)` are deposited by 1F `therefore1.078` will be deposited by 0.01 F=965C (ii) `2H_(2)Oto4H^(+)+O_(2)+4E^(-)` on each electrode 4F LIBERATED 32g `O_(2) therefore0.01F` will liberate `O_(2)=0.08g` `O_(2)` liberated on both electrodes=`=2xx0.08g=0.16`G.