What mass of silver (Atomic mass = 108 g/mol) deposited by a quantity of electricity which displaces 5600 mL of O ₂ at STP ?

Step-by-step solution

Volume of O₂ displaced at STP = 5600 mL = 5.6 L. Moles of O₂ = 5.6 22.4 = 0.25 mol. The reaction for the liberation of O₂ is: 2H₂O O₂ + 4H^+ + 4e^- Number of moles of electrons (Faradays) required for 0.25 mol of O₂ = 0.25 4 = 1 F. The reaction for the deposition of silver is: Ag^+ + e^- Ag Since 1 F of electricity deposits 1 mole of Ag, the mass of Ag deposited is: 1 108 = 108.0 g. Answer: 108.0 g