Tro - Chemistry: A Molecular Approach 6th Edition - Chapter 20

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Ch.20 - Electrochemistry

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Tro 6th Edition

Ch.20 - Electrochemistry

Problem 91b
Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. b. Sn
Problem 91c
Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. c. Mn
Problem 92a
Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. a. Mg
Problem 92b
Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. b. Cr
Problem 92c
Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. c. Cu
Problem 93b
Consider the electrolytic cell: b. Indicate the direction of electron flow.
Problem 94
Draw an electrolytic cell in which Mn²⁺ is reduced to Mn and Sn is oxidized to Sn²⁺. Label the anode and cathode, indicate the direction of electron flow, and write an equation for the half-reaction occurring at each electrode. What minimum voltage is necessary to drive the reaction?
Problem 95
Write equations for the half-reactions that occur in the electrolysis of molten potassium bromide.
Problem 96
What products are obtained in the electrolysis of molten NaI?
Problem 97
Write equations for the half-reactions that occur in the electrolysis of a mixture of molten potassium bromide and molten lithium bromide.
Problem 98
What products are obtained in the electrolysis of a molten mixture of KI and KBr?
Problem 100a
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)
Problem 101
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.
Problem 102
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?
Problem 103
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?
Problem 104
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?
Problem 105
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?
Problem 106
What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt using a current of 25 A?
Problem 107
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.
Problem 108
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 E_cell 𝚫G_rxn
1.00 1.00
1.00 1.00 × 10^-5
1.00 × 10^-5 1.00
4.18 × 10^-4 1.00
Problem 109
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.
Problem 110
Consider the unbalanced redox reaction: Cr₂O₇^2-(aq) + Cu(s) → Cr³⁺(aq) + Cu²⁺(aq) Balance the equation and determine the volume of a 0.850 M K₂Cr₂O₇ solution required to completely react with 5.25 g of Cu.
Problem 113a
Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. a. 2.15 g Al
Problem 113b
Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. b. 4.85 g Cu
Problem 113c
Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. c. 2.42 g Ag
Problem 114
Determine if HNO₃ can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HNO3 and determine the minimum volume of 6.0 M HNO3 required to completely dissolve the sample. a. 5.90 g Au b. 2.55 g Cu c. 4.83 g Sn
Problem 115
The cell potential of this electrochemical cell depends on the pH of the solution in the anode half-cell. Pt(s) | H₂(g, 1 atm) | H⁺(aq, ? M) || Cu²⁺(aq, 1.0 M) | Cu(s) What is the pH of the solution if E_cell is 355 mV?
Problem 116
The cell potential of this electrochemical cell depends on the gold concentration in the cathode half-cell. Pt(s) | H₂(g, 1.0 atm) | H⁺(aq, 1.0 M) || Au³⁺(aq, ? M) | Au(s) What is the concentration of Au³⁺ in the solution if E_cell is 1.22 V?
Problem 117
A friend wants you to invest in a new battery she has designed that produces 24 V in a single voltaic cell. Why should you be wary of investing in such a battery?
Problem 119a
A battery relies on the oxidation of magnesium and the reduction of Cu²⁺. The initial concentrations of Mg²⁺ and Cu²⁺ are 1.0 × 10^–4 M and 1.5 M, respectively, in 1.0-liter half-cells. a. What is the initial voltage of the battery?