To calculate the weight of silver displaced, we need to follow the given steps:



The amount of electricity required to displace 5600 ml of O2 at STP can be calculated using Faraday's laws of electrolysis:

1 mole of electrons = 1 Faraday = 96500 C

1 mole of O2 at STP = 22.4 L = 22400 ml

1 mole of O2 requires 4 moles of electrons to form (from the balanced chemical equation)

Therefore, the amount of electricity required to displace 5600 ml of O2 at STP can be calculated as:

Amount of electricity = (5600/22400) x 4 x 96500 C

Amount of electricity = 48400 C



The amount of silver displaced can be calculated using the equation:

Amount of silver displaced = (Amount of electricity/charge on 1 mole of electrons) x (atomic weight of silver/valency of silver)

The charge on 1 mole of electrons = 1 Faraday = 96500 C

The valency of silver = 1 (since it is a monovalent cation)

Therefore, the amount of silver displaced can be calculated as:

Amount of silver displaced = (48400/96500) x (108/1)

Amount of silver displaced = 54.12 g



The weight of silver displaced by a quantity of electricity which displaces 5600 ml of O2 at STP is 54.12 g.