Chapter 18 – Electrochemistry
35.
The overall reaction 2Co3+(aq) + 2Cl–(aq) → 2Co2+(aq) + Cl2(g) has the standard cell voltage Ecell= 0.46 V. Given E = 1.36
V for the reaction Cl2(g) + 2e– → 2Cl–(aq), calculate the standard reduction potential for the following the half reaction at
25C:
Co3+ + e– → Co2+
36.
An electrochemical cell based on the following reaction has a standard cell voltage (Ecell) of 0.48 V:
Sn(s) + Cu2+(aq) → Sn2+(aq) + Cu(s)
What is the standard reduction potential of tin(II)? (E(Cu2+/Cu) = 0.34 V)
Chapter 18 – Electrochemistry
37.
Consider a voltaic cell based on the following cell reaction:
Ni(s) + At2(s) → Ni2+(aq) + 2At– (aq)
Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine? [E(Ni2+/Ni) = –0.25 V]
Chapter 18 – Electrochemistry
38. Which one of the following reactions will occur spontaneously at standard-state
conditions and 25C?
Chapter 18 – Electrochemistry
39. Which one of the following reactions will occur spontaneously at standard-state
conditions and 25C?
Chapter 18 – Electrochemistry
40.
Consider the following standard reduction potentials in acid solution:
The strongest reducing agent among those shown above is
Chapter 18 – Electrochemistry
41.
Consider the following standard reduction potentials in acid solution:
The strongest oxidizing agent among those shown above is
Chapter 18 – Electrochemistry
42.
Consider the following standard reduction potentials in acid solution:
Which is the weakest oxidizing agent in this list?
Chapter 18 – Electrochemistry
43.
Consider the following standard reduction potentials in acid solution:
The weakest reducing agent listed above is
Chapter 18 – Electrochemistry
44.
Consider the following standard reduction potentials in acid solution:
The strongest reducing agent listed above is
Chapter 18 – Electrochemistry
45.
Consider the following standard reduction potentials in acid solution:
The strongest oxidizing agent listed above is
46. Using a table of standard electrode potentials, decide which of the following statements is
completely true.
Chapter 18 – Electrochemistry
47. Which one of the following reagents is capable of reducing Cu2+(1 M) to Cu(s)?
48. Which one of the following reagents is capable of oxidizing Br– (aq) to Br2(l) under
Chapter 18 – Electrochemistry
49. Which one of the following reagents is capable of oxidizing Cu(s) to Cu2+ (1 M)?
50. Which one of the following reagents is capable of reducing Fe3+ (1 M) to Fe2+ (1 M)?
Chapter 18 – Electrochemistry
51.
The half-cell reaction for the oxidation of H2O(l) to O2(g) is given below.
2H2O(l) → O2(g) + 4H+(aq) + 4e–
Which choice lists all of the following species that can oxidize H2O to O2(g) under standard-state conditions?
MnO4–(aq), Cl2(g), Pb2+(aq), Cl– (aq), Ag+(aq)
52.
Consider the following reaction: 2Fe2+(aq) + Cu2+ → 2Fe3+(aq) + Cu.
When the reaction comes to equilibrium, what is the cell voltage?
Chapter 18 – Electrochemistry
53.
Determine the equilibrium constant, Keq, at 25C for the reaction
2Br– (aq) + I2(s) Br2(l) + 2I– (aq).
54.
Determine the equilibrium constant (Keq) at 25C for the reaction
Cl2(g) + 2Br– (aq) 2Cl– (aq) + Br2(l).
Chapter 18 – Electrochemistry
55.
Given the following standard reduction potentials,
calculate the solubility product of AgCN at 25C.
Chapter 18 – Electrochemistry
56.
Given the following standard reduction potentials,
calculate the formation constant of Ag(NH3)2+ at 25C.
57. For the electrochemical cell, Cd(s) | Cd2+(aq) || Co2+(aq) | Co(s), determine the equilibrium
constant (Keq) at 25C for the reaction that occurs.
Chapter 18 – Electrochemistry
58. For the electrochemical cell, Fe(s) | Fe2+(aq) || Cu2+(aq) | Cu+(aq) | Pt(s), determine the
59.
Calculate G for the electrochemical cell Pb(s) | Pb2+(aq) || Fe3+(aq) | Fe2+(aq) | Pt(s).
Chapter 18 – Electrochemistry
60.
Calculate G for the electrochemical cell Fe(s) | Fe2+(aq) || Sn4+(aq) | Sn2+(aq) | Pt(s).
Subtopic: Standard Reduction (Cell) Potentials
Topic: Electrochemistry
61. For the electrochemical cell Ni(s) | Ni2+(1 M) || H+(1 M) | H2(1 atm) | Pt(s), which one of
the following changes will cause a decrease in the cell voltage?
Chapter 18 – Electrochemistry
62. For the electrochemical cell Pt(s) | H2(1 atm) | H+(1 M) || Cu2+(1 M) | Cu(s), which one of
the following changes will cause an increase in the cell voltage?
63.
Calculate the cell emf for the following reaction at 25C:
2Ag+(0.010 M) + H2(1 atm) → 2Ag(s) + 2H+(pH = 10.0)
Chapter 18 – Electrochemistry
64.
Calculate the cell emf for the following reaction at 25C:
Ni(s) + 2Cu2+(0.010 M) → Ni2+(0.0010 M) + 2Cu+(1.0 M)
65.
Calculate the cell emf for the following reaction:
Cu2+(0.10 M) + H2(1 atm) → Cu(s) + 2H+(pH = 3.00)