ELECTROLYTIC CELL SHORT QUIZ

Electrolytic cells use _______ reaction .

• non spontaneous redox

• spontaneous redox

In an electrolytic cell the electrode at which the electrons enter the solution is called the ______ ; the chemical change that occurs at this electrode is called _______.

• anode, oxidation

• anode, reduction

• cathode, oxidation

• cathode, reduction

Electrical energy is converted to Chemical energy in .........

• A Voltaic Cell

• Both Voltaic and Electrolytic cells

• A Electrolytic Cell

What is the name given to the solution that is being electrolyzed?

• Salt solution

• Mineral solution

• Electric solution

• Electrolyte

What is the coefficient of the bromide ion when the following redox equation is balanced?

BrO^- + Fe(OH)₂ ^__> Br^- + Fe(OH)₃

• 1

• 2

• 3

• 4

What is the product formed at the cathode in the electrolysis of molten NaCl?

• Chlorine gas

• Sodium metal

• Hydrogen gas

• Oxygen gas

The anode half equation is _______________.(a) 2Br^-(l) --> Br₂(g) + e(b) 2Br^-(l) --> Br₂(l) + 2e(c) Zn²⁺(l) + 2e--> Zn(s)(d) Zn²⁺(l) + 2e --> Zn(l)

• 2Br^-(l) --> Br₂(g) + e

• 2Br^-(l) --> Br₂(l) + 2e

• Zn²⁺(l) + 2e--> Zn(s)

• Zn²⁺(l) + 2e --> Zn(l)

How much voltage will you have to apply to carry out this reaction?

• Less than 1.1V

• No voltage needs to be applied because this reaction represents an electrolytic cell

• Greater than 1.1V

• No voltage needs to be applied because this reaction represents a galvanic cell

The half-reaction that occurs at the anode during the electrolysis of molten sodium bromide is:

• 2 Br^- --> Br₂ + 2 e^-

• Br₂ + 2 e^- --> 2 Br^-

• Na⁺ + e^- --> Na

• Na --> Na⁺ + e^-

How long (in hours) must a current of 5.0 amperes be maintained to electroplate 60 g of calcium from molten CaCl₂?

• 27 hours

• 8.3 hours

• 11 hours

• 16 hours