Textbook Question
Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution. a. Ni(NO3)2(aq)
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Ch.19 - Electrochemistry
Chapter 19, Problem 99
Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction: Cu2+(aq) + 2 e- → Cu(s). How much time would it take for 325 mg of copper to be plated at a current of 5.6 A?
Verified step by step guidance1
Convert the mass of copper from milligrams to grams by dividing by 1000.
Calculate the number of moles of copper using its molar mass (63.55 g/mol).
Use the stoichiometry of the half-reaction to determine the moles of electrons required. Since 1 mole of Cu requires 2 moles of electrons, multiply the moles of Cu by 2.
Apply Faraday's Law of Electrolysis: Q = n * F, where Q is the total charge in coulombs, n is the moles of electrons, and F is Faraday's constant (96485 C/mol).
Calculate the time using the formula t = Q / I, where t is time in seconds, Q is the total charge, and I is the current (5.6 A).
Related Practice
Textbook Question
Make a sketch of an electrolysis cell that electroplates copper onto other metal surfaces. Label the anode and the cathode and indicate the reactions that occur at each.
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Open Question
How can one sketch an electrolysis cell that electroplates nickel onto other metal surfaces, labeling the anode and cathode and indicating the reactions that occur at each?
Textbook Question
Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag+(aq) + e– → Ag(s) What mass of silver would plate onto the cathode if a current of 6.8 A flowed through the cell for 72 min?
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Textbook Question
A major source of sodium metal is the electrolysis of molten sodium chloride. What magnitude of current produces 1.0 kg of sodium metal in 1 hour?
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Open Question
What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt using a current of 25 A?