Problem- 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 96,500 coulombs (C) and 1 ampere (A) = 1 coulomb/second (C/s)
1. What mass of Cu(s) is electroplated by running 18.5A of current through a Cu2+(aq) solution for 4.00 h?
2. How many minutes will it take to electroplate 55.1g of gold by running 5.00 A of current through a solution of Au+(aq)?
Please illustrate work if possible want to understand, not just receive answers