A jeweler needs to electroplate gold onto a bracelet using an ionic solution. He knows that the charge carriers in the ionic solution are gold ions of charge e, and that each gold ion has a mass of 22g. The gold ions move through the solution, and are deposited on the bracelet. He has calculated that he must deposit 0.20 g of 901d to reach the necessary thickness. If each gold ion has a mass of g, what current should he use to electroplate the bracelet in three hours

Explanation:

First, we will calculate the total charge as follows.

                    =

                    = 97.80 C

Now, we will calculate the current required by the jeweler to plate the bracelet as follows.

                   i =

                     =

                     = A

or,                  = 9.05 mA

thus, we can conclude that 9.05 mA current should he use to electroplate the bracelet in three hours.

pythagoras' theorem

square root (-5^2+9^2)

square root (25+81)

square root (106)

angle is tan^-1(9/5)

neg x, pos y