Ch.20 - Electrochemistry

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Tro 5th Edition

Ch.20 - Electrochemistry

Problem 37a,b

Balance each redox reaction occurring in acidic aqueous solution. a. K(s) + Cr³⁺(aq) → Cr(s) + K⁺(aq) b. Al(s) + Fe²⁺(aq) → Al³⁺(aq) + Fe(s)

Problem 37c

Balance each redox reaction occurring in acidic aqueous solution. c. BrO₃^–(aq) + N₂H₄(g) → Br^–(aq) + N₂(g)

Problem 38b

Balance each redox reaction occurring in acidic aqueous solution. b. Mg(s) + Cr³⁺(aq) → Mg²⁺(aq) + Cr(s)

Problem 38c

Balance each redox reaction occurring in acidic aqueous solution. c. MnO₄^–(aq) + Al(s) → Mn²⁺(aq) + Al³⁺(aq)

Problem 40a

Balance each redox reaction occurring in acidic aqueous solution. a. I^–(aq) + NO₂^–(aq) → I₂(s) + NO(g) b. ClO₄^–(aq) + Cl^–(aq) → ClO₃^–(aq) + Cl₂(g)

Problem 42a

Balance each redox reaction occurring in basic aqueous solution. a. MnO₄^–(aq) + Br^–(aq) → MnO₂(s) + BrO₃^–(aq)

Problem 42c

Balance each redox reaction occurring in basic aqueous solution. c. NO₂^–(aq) + Al(s) → NH₃(g) + AlO₂^–(aq)

Problem 46

Calculate the standard cell potential for each of the electrochemical cells in Problem 44.

Problem 47d

Consider the voltaic cell:

d. Indicate the direction of anion and cation flow in the salt bridge

Problem 49

Use line notation to represent each electrochemical cell in Problem 43.

Problem 52

Is the question formulating correctly? If yes, return the question without changes. If not, please fix it and return the output as a JSON of the form: {'question': 'question text'}. Here is the question: Make a sketch of the voltaic cell represented by the line notation. Write the overall balanced equation for the reaction and calculate E°cell. Mn(s) | Mn2+(aq) || ClO2-(aq) | ClO2(g) | Pt(s)

Problem 53

Determine whether or not each redox reaction occurs spontaneously in the forward direction.

a. Ni(s) + Zn²⁺(aq) → Ni²⁺(aq) + Zn(s)

b. Ni(s) + Pb²⁺(aq) → Ni²⁺(aq) + Pb(s)

c. Al(s) + 3 Ag⁺(aq) → Al³⁺(aq) + 3 Ag(s)

d. Pb(s) + Mn²⁺(aq) → Pb²⁺(aq) + Mn(s)

Problem 54

Determine whether or not each redox reaction occurs spontaneously in the forward direction.

a. Ca²⁺(aq) + Zn(s) → Ca(s) + Zn²⁺(aq)

b. 2 Ag⁺(aq) + Ni(s) → 2 Ag(s) + Ni²⁺(aq)

c. Fe(s) + Mn²⁺(aq) → Fe²⁺(aq) + Mn(s)

d. 2 Al(s) + 3 Pb²⁺(aq) → 2 Al³⁺(aq) + 3 Pb(s)

Problem 55

Which metal could you use to reduce Mn²⁺ ions but not Mg²⁺ ions?

Problem 56

Which metal can be oxidized with an Sn²⁺ solution but not with an Fe²⁺ solution?

Problem 57

Determine whether or not each metal dissolves in 1 M HCl. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Al b. Ag c. Pb

Problem 59

Determine whether or not each metal dissolves in 1 M HNO₃. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Cu b. Au

Problem 60

Determine whether or not each metal dissolves in 1 M HIO₃. For those metals that do dissolve, write a balanced redox equation for the reaction that occurs. a. Au b. Cr

Problem 61a

Calculate E°_cell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. 2 Cu(s) + Mn²⁺(aq) → 2 Cu⁺(aq) + Mn(s)

Problem 61b,c

Calculate E°_cell for each balanced redox reaction and determine if the reaction is spontaneous as written. b. MnO₂(aq) + 4 H⁺(aq) + Zn(s) → Mn²⁺(aq) + 2H₂O(l) + Zn²⁺(aq) c. Cl₂(g) + 2 F^–(aq) → F₂(g) + 2 Cl^–(aq)

Problem 62a,b

Calculate E°_cell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. O₂(g) + 2 H₂O(l) + 4 Ag(s) → 4 OH^–(aq) + 4 Ag⁺(aq) b. Br₂(l) + 2 I^–(aq) → 2 Br^–(aq) + I₂(s)

Problem 62c

Calculate E°_cell for each balanced redox reaction and determine if the reaction is spontaneous as written. c. PbO₂(s) + 4 H⁺(aq) + Sn(s) → Pb²⁺(aq) + 2 H₂O(l) + Sn²⁺(aq)

Problem 63

Which metal cation is the best oxidizing agent? a. Pb²⁺ b. Cr³⁺ c. Fe²⁺ d. Sn²⁺

Problem 65b,c

Use tabulated electrode potentials to calculate ∆G°_rxn for each reaction at 25 °C. b. Br₂(l) + 2 Cl^–(aq) → 2 Br^–(aq) + Cl₂(g) c. MnO₂(s) + 4 H⁺(aq) + Cu(s) → Mn²⁺(aq) + 2 H₂O(l) + Cu²⁺(aq)

Problem 66

Use tabulated electrode potentials to calculate ∆G°rxn for each reaction at 25 °C. a. 2 Fe³⁺(aq) + 3 Sn(s) → 2 Fe(s) + 3 Sn²⁺(aq) b. O₂(g) + 2 H₂O(l) + 2 Cu(s) → 4 OH^–(aq) + 2 Cu²⁺(aq) c. Br₂(l) + 2 I^–(aq) → 2 Br^–(aq) + I₂(s)

Problem 67

Calculate the equilibrium constant for each of the reactions in Problem 65.

Problem 69

Calculate the equilibrium constant for the reaction between Ni2+(aq) and Cd(s) at 25 °C.

Problem 70

Calculate the equilibrium constant for the reaction between Fe²⁺(aq) and Zn(s) (at 25 °C).

Problem 71

Calculate ΔG°_rxn and E°_cell for a redox reaction with n = 2 that has an equilibrium constant of K = 25 (at 25 °C).

Problem 73

A voltaic cell employs the following redox reaction: Sn²⁺(aq) + Mn(s) → Sn(s) + Mn²⁺(aq) Calculate the cell potential at 25 °C under each set of conditions. c. [Sn²⁺] = 2.00 M; [Mn²⁺] = 0.0100 M