38 . 6 amperes of current is passed for 100 seconds through an aqueous CuSO 4 solution using platinum electrodes. The mass of copper consumed from the solution and volume of gas liberated at STP are respectively (molar mass of Cu = 63 . 54 gmol - 1 )

Step-by-step solution

Reduction potential of Cu 2+ is higher than H + hence Cu 2+ will be reduced at cathode more easily. Reaction at the cathode: Cu + 2 + 2 e - → Cu Reaction at the Anode: 2 H 2 O → O 2 + 4 H + + 4 e - According to Faraday's first law W = Zit W = E 96500 it W = Atomic   weight   of   Cu n × 96500 it     = 63 . 54 2 × 96500 × 38 . 6 × 100       = 1 . 27 g When 63.54 grams of copper deposited 11.2 litres of oxygen gas is released at anode. Hence,