A Jeweler Needs to Electroplate Gold,having an Atomic Mass of 196.97

A jeweler needs to electroplate gold,having an atomic mass of 196.97 g/mol,onto a bracelet.He knows that the charge carriers in the ionic solution are singly-ionized gold ions,Au⁺,and has calculated that he must deposit $0.20 \mathrm {~g}$ of gold to reach the necessary thickness.How much current does he need to plate the bracelet in 3.0 hours? (e = 1.60 × 10^-19 C,N_A = 6.02 × 10²³ atoms/mol)

A) 9.1 mA
B) 540 mA
C) 33 A
D) 1800 mA

Correct Answer:

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