A silver electroplating process is 80% efficient. Calculate the mass of silver deposited on an object when 2.0 Faradays of charge are passed through a silver nitrate (AgNO3) solution.
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To calculate the mass of silver deposited on an object, we need to convert the charge passed through the solution into moles of silver, and then into mass.
First, we need to find the number of moles of silver that corresponds to 2.0 Faradays of charge. Faraday's constant is 96,485 C/mol e-.
2.0 Faradays x 96,485 C/mol e- = 192,970 C
Next, we need to convert the charge in Coulombs into moles of electrons. The charge of each electron is 1.6 x 10^-19 C.
192,970 C x (1 mol e- / 1.6 x 10^-19 C) = 1.205 x 10^15 mol e-
Since the silver electroplating process is 80% efficient, only 80% of the moles of electrons correspond to the moles of silver deposited.
80% of 1.205 x 10^15 mol e- = 9.64 x 10^14 mol Ag
Finally, we need to convert the moles of silver into mass. The molar mass of silver is 107.87 g/mol.
9.64 x 10^14 mol Ag x 107.87 g/mol = 1.04 x 10^17 g
Therefore, the mass of silver deposited on the object is approximately 1.04 x 10^17 grams.
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