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
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)

Question

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

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)

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