Suppose that you planned to goldplate a medallion using a 05

Suppose that you planned to gold-plate a medallion using a 0.500M soltion of Au(no3)3 using a current of 0.50 amps over a period of 3 hours.

A. How many grams of gold would plate on the metal used for the medallion?

B. How much 0.500M Au(no3)3 solution would you need to prepare to accomplish this?

C. What is the mass of gold transferred to the medallion?

a) we know that m= zQ

z= electro chemical equivalent of gold

= 2.4496g/amp-h

so m= 2.4496* 0.50* 3

=3.6744 g

b) moles of gold deposited= 3.6744/197

=0.018 moles

so molarity of Au (no3)3= 0.5

so 0.018/V= 0.5

V= 36 ml

c) mass of gold transferred= 3.6744 g