Chemistry: Quiz: Faraday's Laws

Quiz: Faraday's Laws

1. __________ use an externally generated electrical current to produce a chemical reaction that would not otherwise take place.

a. Voltaic cells

b. Electrolytic cells

c. Salt bridges

2. The fundamental quantity of electrical charge on one mole of electrons used by chemists is a

a. Faraday

b. pooraday

c. volt

3. Michael Faraday found that the mass of a substance produced by a redox reaction at an electrode is __________ the quantity of electrical charge that has passed through the electrochemical cell.

a. less than

b. the square root of

c. proportional to

4. The charge on one mole of electrons is __________ Coulombs.

a. 186000

b. 96500

c. 0.05916

5. Consider the reduction of Mn⁷⁺ to Mn²⁺. How many Faradays of electrical charge are needed?

a. 2

b. 7

c. 5

6. The electrolysis of a sample of LiBr yielded 20.82 grams of lithium when 3.0 Faradays of electricity were passed through the sample. What was the mass of the sample?

a. 20.82 grams

b. 260.5 grams

c. 239.7 grams

7. A conclusion from Faraday's second law is that for a given quantity of electricity, the moles of substance produced __________ as the oxidation number increases.

a. increases

b. is equivalent

c. decreases

8. The electrolysis of water produces

a. gaseous water

b. H₂ and O₂ gases

c. electrically charged water

9. Electrolysis uses electrical current to

a. speed up a spontaneous reaction

b. force a nonspontaneous reaction to occur

c. stop a spontaneous reaction from proceeding