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1. Rusting occurs due to the oxidation–reduction reaction of iron with environmental oxygen:
4 Fe (s) + 3 O2 (g) → 2 Fe2O3 (s)
Some metals cannot react with oxygen in this fashion.
Which of the following best explains why iron can?
2. Given the following standard reduction potentials:
What is the standard electromotive force of the following reaction?
Zn2+ + 2 Ag → 2 Ag+ + Zn
3. Consider the following data:
The anode of a certain galvanic cell is composed of copper. Which of the metals from the data table can be used at the cathode, assuming equal concentrations of the two electrolyte solutions?
4. An electrolytic cell is filled with water. Which of the following will move toward the cathode of such a cell?
I. H+ ions
II. O2– ions
5. If the value of E°cell is known, what other data is needed to calculate ΔG°?
6. Which of the following compounds is LEAST likely to be found in the salt bridge of a galvanic cell?
7. If the surface area of electrode material in an electrochemical cell is tripled, what else is necessarily tripled?
8. Which of the following can alter the emf of an electrochemical cell?
9. Which of the following statements could be true about a Na–Cd cell, based on the information below?
10. Which of the following expressions correctly describes the relationship between standard electromotive force and standard change in free energy?
11. Which of the following choices is indicative of a spontaneous reaction, assuming standard condition?
12. For a cell with the following half-reactions:
Anode: SO2 + 2 H2O → SO42- + 4 H+ + 2 e-
Cathode: Pd2+ + 2 e- → Pd
How would decreasing the pH of the solution inside the cell affect the electromotive force (emf)?
13. An electrolytic cell necessarily has:
14. Which of the following is the best explanation for the fact that a larger mass of electrodes are required for lead–acid batteries, as compared to other batteries, to produce a certain current?
15. Which of the following best describes why over-charging a Ni–Cd battery is not detrimental?
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