Self Quiz Answers

1. Which of the following chemicals can be oxidized most easily?

*a. Na
b. Mg
c. Cl₂
d. F^-
e. Al³⁺

2. Which of the following is/are oxidation-reduction reactions?

a. Mg + 2H⁺ Mg²⁺ + H₂
b. N₂ + O₂ 2NO
c. NaCl + AgNO₃ AgCl + NaNO₃
*d. (a) and (b)
e. (a), (b) and (c)

3. Oxidation and reduction must take place at the same time because electrons are:

a. gained.
b. lost.
*c. transferred.

4. What voltage could a cell generate (under ideal conditions) using the following reaction?

3 Mg + 2 AlCl₃ 3 MgCl₂ + 2 Al

a. -4.03 v
b. -0.71 v
*c. +0.71 v
d. +3.79 v
e. +4.03 v

5. Electrolytic cells:

1. can be used to force reactions that do not occur spontaneously.
2. need an external source of electricity.
3. can be used for electroplating.

a. only one of these
b. 1 and 2
c. 1 and 3
d. 2 and 3
*e. all of these

6. Which of the following combinations will react in a spontaneous oxidation-reduction reaction?

a. Zn + Zn²⁺
b. Cr + Fe
*c. Cd + Ni²⁺
d. Sn + Fe²⁺
e. Ag⁺ + Br₂

7. The gain of electrons is called:

a. oxidation.
b. oxidation-reduction.
c. redox.
*d. reduction.
e. none of the above.

8. If two copper electrodes are put into a silver nitrate solution and a current is run through the cell, what will happen at the anode?

a. Copper will plate out.
b. Silver will plate out.
*c. Copper will go into solution.
d. Silver will go into solution.

9. In what kind of cell would this reaction occur?

2 Al + 3 CuCl₂ 2 AlCl₃ + 3 Cu

a. anodic
b. cathodic
c. electrolytic
d. hypnotic
*e. voltaic

10. Diagram a voltaic cell using this reaction:  Ni + Pb²⁺ Pb + Ni²⁺.

Indicate the placement of the chemicals, the location of the electron flow, and the half reaction occurring at each electrode.

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