"bar of gold or copper placed in acidic solution, attached via battery to item to be plated. Eyeglasses plated placed in solution, voltage applied to create electrolytic cell, which plates material." 1. Total amount of gold to deposit on glasses made of aluminum = 0.5g. How long should the plating process be performed to deposit this amount of gold? 2. If the glasses are plated with copper instead of gold... A) Reaction require lower V, proceed at same speed for equal current B) Reaction require lower V, but proceed more quickly C) Reaction require same voltage but proceed slowly for equal current Reduction potentials: Au3+ + 3e --> Au 1.5V Cu2+ + 2e --> Cu 0.34V Al3+ + 3e --> Al 1.66V Attempts: 1. 0.5g x (1mol/197gAu) x (3e-/1mole) x (96487C/mole) x 1s/C = ~730s However, answer is 73s because the last term they did is 1s/10C. How come? 2. I was thinking that the reaction would require a higher voltage since the difference between the reduction potential of Al and Cu is greater than the difference between Al and Au. Thank you.