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- Arrange the following oxidizing agents in order of increasing strength under standard-state conditions: Br2(aq), MnO4+(aq), Sn4+(aq).
Problem 74
- List the following reducing agents in order of increasing strength under standard-state conditions: Al(s), Pb(s), Fe(s).
Problem 75
- Consider the following substances: I2(s), Fe2+(aq), Cr2O72-(aq). Which is the strongest oxidizing agent? Which is the weakest oxidizing agent?
Problem 76
- Consider the following substances: Fe2+(aq), Sn2+(aq), I-(aq). Identify the strongest reducing agent and the weakest reducing agent.
Problem 77
- Consider the following substances: Fe(s), PbO2(s), H+(aq), Al(s), Ag(s), Cr2O72-(aq). (d) Which substances can be oxidized by Cu2+(aq)? Which can be reduced by H2O2(aq)?
Problem 78
Problem 78a
Consider the following substances: Fe(s), PbO2(s), H+(aq), Al(s), Ag(s), Cr2O72-(aq). (a) Look at the E° values in Appendix D, and classify each substance as an oxidizing agent or a reducing agent.
- The following cell reactions occur spontaneously: (c) Which of the three cell reactions delivers the highest voltage?
Problem 79
Problem 79a
The following cell reactions occur spontaneously: (a) Arrange the following reduction half-reactions in order of decreasing tendency to occur:
Problem 79b
The following cell reactions occur spontaneously: (b) Which of these substances (A,A+,B,B+,C,C+) is the strongest oxidizing agent? Which is the strongest reducing agent?
Problem 80a
Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (a) Oxidation of Sn2+(aq) by Br2(aq)
Problem 80b
Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (b) Reduction of Ni2+(aq) by Sn2+(aq)
Problem 80c
Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (c) Oxidation of Ag(s) by Pb2+(aq)
Problem 80d
Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (d) Reduction of I2(s) by H2SO3(aq)
Problem 82a
What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (a) Oxygen gas is bubbled through an acidic solution of Cr(NO3)3.
Problem 82b
What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (b) A strip of lead is dipped into an aqueous solution of AgNO3.
Problem 82c
What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (c) Chlorine gas is bubbled through aqueous H2C2O4.
Problem 82d
What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (d) A nickel wire is dipped into an aqueous solution of HClO.
Problem 83a
What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (a) A strip of zinc is dipped into an aqueous solution of Pb(NO3)2.
Problem 83b
What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (b) An acidic solution of FeSO4 is exposed to oxygen.
Problem 83c
What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (c) A silver wire is immersed in an aqueous solution of NiCl2.
Problem 83d
What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (d) Hydrogen gas is bubbled through aqueous Cd(NO3)2.
- The standard potential for the following galvanic cell is 0.40 V: (Europium, Eu, is one of the lanthanide elements.) Use the data in Table 19.1 to calculate the standard reduction potential for Eu3+/Eu2+ half-cell.
Problem 84
- Calculate E° for each of the following reactions, and tell which are spontaneous under standard-state conditions. (a)
Problem 91
Problem 92b
Consider a galvanic cell that uses the following half-reactions: (b) What is the oxidizing agent, and what is the reducing agent?.
- Given the following half-reactions and E° values, write a balanced equation for the formation of Mn2+ and MnO2 from Mn3+, and calculate the value of E° for this reaction. Is the reaction spontaneous under standard-state conditions?
Problem 93
- Consider a galvanic cell that uses the reaction Calculate the potential at 25 °C for a cell that has the following ion concentrations: [Ag+] = 0.010M, [Ni2+] = 0.100M.
Problem 94
- A galvanic cell has an iron electrode in contact with 0.10 M FeSO4 and a copper electrode in contact with a CuSO4 solu-tion. If the measured cell potential at 25 °C is 0.67 V, what is the concentration of Cu2+ in the CuSO4 solution?
Problem 97
- What is the Fe2+: Sn2+ concentration ratio in the following cell at 25 °C if the measured cell potential is 0.35 V?
Problem 99
- The Nernst equation applies to both cell reactions and half-reactions. For the conditions specified, calculate the potential for the following half-reactions at 25 °C. (b)
Problem 100
Problem 101a
When suspected drunk drivers are tested with a Breathalyzer, the alcohol (ethanol) in the exhaled breath is oxidized to acetic acid with an acidic solution of potassium dichromate: The color of the solution changes because some of the orange Cr2O72- is converted to the green Cr3+ The Breathalyzer measures the color change and produces a meter reading calibrated in blood alcohol content. (a) What is E° for the reaction if the standard half-cell potential for the reduction of acetic acid to ethanol is 0.058 V?