Practice Electrolytic Cell in Chemistry

Use these practice problems to test your method after reviewing the concept explanation and worked examples.

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Quick Recap

An electrolytic cell uses an external power source to force a nonspontaneous redox reaction to occur. Electrical energy is converted into chemical change.

Instead of getting electricity from chemistry, you spend electricity to make chemistry happen.

Showing a random 20 of 50 problems.

Example 1

easy

Is the reaction in an electrolytic cell spontaneous or nonspontaneous?

Example 2

easy

Reduction occurs at which electrode in an electrolytic cell?

Example 3

medium

A current of

2.00

A flows for

30.0

minutes. How many coulombs of charge pass through the cell?

Example 4

medium

Electrolysis of

1.00

L of

1.0

CuSO_4

delivers

0.20

mol of electrons. By how much does

[Cu^{2+}]

decrease?

Example 5

easy

What kind of energy source does an electrolytic cell require?

Example 6

hard

In electroplating, a spoon is to be coated with silver from

AgNO_3

. Which electrode should the spoon be connected to?

Example 7

medium

During electrolysis, do electrons flow through the external wire from anode to cathode or cathode to anode?

Example 8

easy

What does the value of Faraday's constant represent?

Example 9

easy

Does an electrolytic cell work like a battery (power source) or the opposite?

Example 10

challenge

A current of 5.0 A runs for 1930 s through molten

AlCl_3

. How many grams of Al deposit? (Al = 27 g/mol, F = 96500 C/mol)

Example 11

medium

Compare the sign of

\Delta G

for a galvanic versus an electrolytic cell reaction.

Example 12

medium

What is the role of an inert electrode (like platinum) in electrolysis?

Example 13

hard

A constant current deposits

1.50

g of

Ni

(

58.7

g/mol,

Ni^{2+}

) in

30.0

minutes. What is the current in amperes?

Example 14

medium

How many moles of electrons are needed to deposit 1 mol of

Al

from

Al^{3+}

by electrolysis?

Example 15

challenge

A factory needs to produce

1000

kg of aluminum per day by the Hall-Heroult process. What constant current (in amperes) is required? (

Al = 27

g/mol,

F = 96{,}500

C/mol)

Example 16

medium

In electrolysis of aqueous

NaCl

(brine), why is

Cl_2

produced at the anode rather than

O_2

Example 17

easy

In electrolysis of molten

NaCl

, what is the overall cell reaction?

Example 18

medium

How many moles of electrons correspond to

96{,}500

C of charge?

Example 19

hard

At what minimum voltage will electrolysis of water proceed under standard conditions (

E^\circ_{O_2/H_2O} = +1.23

E^\circ_{H^+/H_2} = 0.00

V)?

Example 20

easy

Electrolytic cells convert electrical energy into what?

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Related Concepts

Electrochemical Cell