Practice Electrochemistry in Chemistry

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

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Quick Recap

Electrochemistry is the study of redox reactions that involve electric current, either producing electricity from a spontaneous reaction (a galvanic/voltaic cell) or using electricity to force a nonspontaneous reaction to occur (an electrolytic cell).

Electrochemistry connects chemical reactions and electrical energy in both directions.

Showing a random 20 of 50 problems.

Example 1

easy

E^\circ_{cell} > 0

, what is the sign of

\Delta G^\circ

Example 2

easy

Which device converts chemical energy into electrical energy: a battery or an electrolysis cell?

Example 3

medium

In an electrochemical cell at equilibrium, what is the value of

E_{cell}

Example 4

medium

A cell has

E^\circ_{cell} = +1.10

V. Is the reaction spontaneous, and is the cell galvanic?

Example 5

easy

Does electrolysis use a spontaneous or nonspontaneous reaction?

Example 6

challenge

A galvanic cell has

E^\circ_{cell}=+1.10

V with

n=2

. Compute

\Delta G^\circ

in kJ. (F = 96500 C/mol)

Example 7

easy

Which has the higher reduction potential:

F_2/F^-

(

+2.87

V) or

Li^+/Li

(

-3.04

V)? Which is the better oxidizing agent?

Example 8

medium

Fill in the blank: in a battery during discharge, the cathode is the ____ terminal.

Example 9

easy

In an electrochemical cell, what carries charge through the solution?

Example 10

easy

Identify the oxidized and reduced species in:

Zn + Cu^{2+} \to Zn^{2+} + Cu

Example 11

hard

A student claims electrolysis can run without an external power source. Correct the misconception.

Example 12

medium

A current of

2.00\text{ A}

runs for

1\,930\text{ s}

in an electrolysis of aqueous

CuSO_4

. Find the mass of Cu deposited. (

M(Cu)=63.5\text{ g/mol}

F=96500\text{ C/mol}

)

Example 13

easy

Is corrosion of iron an example of electrochemistry?

Example 14

medium

In the Zn/Cu cell, Zn is oxidized and Cu2+ is reduced. Which metal is the anode?

Example 15

medium

For

E^\circ_{cell} = +0.46

V with

n=2

, find the sign of

\Delta G

using

\Delta G = -nFE^\circ_{cell}

Example 16

easy

In a spontaneous electrochemical cell, electrons flow from which electrode to which?

Example 17

medium

Why are noble gases generally inert in electrochemistry?

Example 18

medium

E^\circ(Cu^{2+}/Cu) = +0.34

E^\circ(Pb^{2+}/Pb) = -0.13

V. Which metal is the better reducing agent?

Example 19

medium

Use

\Delta G^\circ = -nFE^\circ_{cell}

: a galvanic cell has

\Delta G^\circ = -386\text{ kJ}

and

n = 4

. Find

E^\circ_{cell}

. (

F = 96500\text{ C/mol}

)

Example 20

medium

If electrons flow from electrode A to electrode B in the wire, which is the cathode?

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Related Concepts

Redox Reaction Electrolyte Electrochemical Cell Electrolytic Cell