A jeweler wishes to electroplate a brass pendant with exactly (2.50
CHEMISTRY · Multi-part · AP · Chemistry · Thermodynamics and Electrochemistry · Thermodynamics and Electrochemistry
Problem
A jeweler wishes to electroplate a brass pendant with exactly 2.50g of copper in 35.0min. The plating bath contains aqueous Cu2+ ions, and the process operates at 100\% current efficiency. The Faraday constant is 96485C mol−1, and the molar mass of copper is 63.55g mol−1.
(a) Calculate the number of moles of copper that must be deposited.
(b) Determine the total charge, in coulombs, that must pass through the cell to achieve this mass of copper.
(c) Calculate the minimum steady current, in amperes, required to complete the plating in the allotted time.
(d) A power supply capable of delivering a constant 1.50A is available. Evaluate whether this supply can complete the plating within 35.0min, and support your answer with quantitative reasoning.