A Jeweler Needs to Electroplate Gold, Having an Atomic Mass $0.20 \mathrm {~g}$

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:

Verified

Unlock this answer now
Get Access to more Verified Answers free of charge

Access For Free