Open Question
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?
Ch.19 - Electrochemistry
Chapter 19, Problem 102
What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt using a current of 25 A?
Verified step by step guidance1
Identify the relevant electrochemical reaction: The reduction of aluminum ions to aluminum metal is represented by the half-reaction: \( \text{Al}^{3+} + 3e^- \rightarrow \text{Al} \).
Determine the number of moles of electrons required: From the half-reaction, 3 moles of electrons are needed to produce 1 mole of aluminum.
Use Faraday's Law of Electrolysis: The amount of substance produced at an electrode is directly proportional to the quantity of electricity passed through the electrolyte. The formula is \( n = \frac{I \cdot t}{n_e \cdot F} \), where \( n \) is the number of moles of aluminum, \( I \) is the current in amperes, \( t \) is the time in seconds, \( n_e \) is the number of moles of electrons, and \( F \) is Faraday's constant (approximately 96485 C/mol).
Calculate the time in seconds for one hour: Since the problem asks for the mass produced per hour, convert 1 hour into seconds (1 hour = 3600 seconds).
Calculate the mass of aluminum produced: Use the molar mass of aluminum (approximately 26.98 g/mol) to convert the moles of aluminum to grams.
Related Practice
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?
1055
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Open Question
Consider the reaction shown here occurring at 25 °C: A(s) + B2+(aq) → A2+(aq) + B(s). Given that ∆Gr°xn = -14.0 kJ, determine the value of Ec°ell and K for the reaction, and complete the following table for [B2+], [A2+], Q, Ecell, and ∆Grxn with initial values 1.00, 1, 1.0 * 10^-4, 3.54 * 10^-3, and 1.00 * 10^-4 respectively.
Textbook Question
Consider the reaction shown here occurring at 25°C. Cr(s) + Cd2+(aq) → Cr2+(aq) + Cd(s) Determine E°cell, K, and ∆G°rxn for the reaction and complete the table.
[Cd2+] [Cr2+] Q Ecell 𝚫Grxn
1.00 1.00
1.00 1.00 × 10-5
1.00 × 10-5 1.00
4.18 × 10-4 1.00
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Open Question
Consider the unbalanced redox reaction: MnO4-(aq) + Zn(s) → Mn2+(aq) + Zn2+(aq). Balance the equation and determine the volume of a 0.500 M KMnO4 solution required to completely react with 2.85 g of Zn.