Copper is electroplated from CuSO₄ solution.A constant current of 3.19 amp is applied by an external power supply.How long will it take to deposit 1.00 $\times$ 10² g of Cu? The atomic mass of copper is 63.546.

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The correct answer is A.The amount of substance deposited is given by the equation:$$m = \frac{It}{nF}$$where:* m is the mass of the substance deposited (in grams)* I is the current (in amperes)* t is the time (in seconds)* n is the number of moles of electrons transferred per mole of substance deposited* F is the Faraday constant (96,485 C/mol)In this case, we have:* m = 1.00 g* I = 3.19 A* n = 2 (since Cu2+ ions are being reduced to Cu)* F = 96,485 C/molSolving for t, we get:$$t = \frac{m n F}{I}$$$$t = \frac{(1.00 g)(2 mol/electron)(96,485 C/mol)}{3.19 A}$$$$t = 26.4 h$$

Copper Is Electroplated from CuSO4 Solution ×\times× 102 G of Cu? the Atomic Mass of Copper Is

Copper Is Electroplated from CuSO₄ Solution $\times$ 10² G of Cu? the Atomic Mass of Copper Is