Question

Part A and B

Please show all of the steps

Analysis of Electroplating When electricity (the flow of electrons) is passed through a solution, it causes an oxidation-reduction (redox) reaction to occur. If the solution contains a metal cation such as Ag+, the flow of electrons will reduce the silver ion, causing solid silver to plate onto the electrode. The amount of metal plated depends on the number of electrons passed. The total charge of a mole of electrons is 96,485 coulombs (C) and 1 ampere (A) = 1 coulomb/ second (C/s)

Answer 1

Cu2+ cas, trê – Cu(s) to deposit I mole or We require af or 2x 96485c 63 g of cu convert time in seconds) t = 4x 60 x 60s t = 14,4005 charge = current y time = 20.0x 14, 400 = 288,oooc deposit 2 x 96 485 c 63 g cu 63 g cu 2 x 9 6485 288,00oC 6 x 288000 g cu 2 x 9 6485 = 94.02 g cu so 94.02 g cu will be electroplated

Auteag.) + 2 – Alu (s) If or 96485c to deposit we require of Au 197g or Imole require 1979 require 9 6485 c 19 - 96485 197 24.1g 9 6485 x 24.1c 197 = 11803. 5c charge is required to So 11803.50 24.12 Au electroplate charge = current & time 11803.5 = 5.0x time time = 2360.7 sec or time = 2360.7 Go sec = 1 minute / time = 39. 34 minutes