Practice Electrochemical 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 electrochemical cell is a system with two half-reactions separated into electrodes and connected through an external circuit so electrons can flow.

Separate the oxidation and reduction halves, connect them with a wire and ion path, and the reaction can do electrical work.

Showing a random 20 of 50 problems.

Example 1

easy

Reduction occurs at which electrode of an electrochemical cell?

Example 2

easy

In an electrochemical cell, what flows through the external wire?

Example 3

medium

In a galvanic cell, which direction do anions migrate in the salt bridge?

Example 4

medium

In a galvanic cell, which direction do cations from the salt bridge migrate, and why?

Example 5

challenge

In a

Zn/Cu

cell with

E^\circ_{cell}=1.10

V, 0.50 mol of electrons pass. Find the maximum electrical work. (F = 96500 C/mol)

Example 6

challenge

Given

Ag^+ + e^- \rightarrow Ag

(

+0.80

V) and

Cu^{2+} + 2e^- \rightarrow Cu

(

+0.34

V), determine the cathode and

E^\circ_{cell}

Example 7

hard

A current of

1.50\text{ A}

flows for

600\text{ s}

through an electrochemical cell electroplating Ag from

Ag^+

. Find the mass of Ag deposited. (

F = 96500\text{ C/mol}

M(Ag) = 108\text{ g/mol}

)

Example 8

easy

True or false: in a galvanic cell, electrons leave the cathode and travel to the anode through the external wire.

Example 9

easy

What are the two electrodes in an electrochemical cell called?

Example 10

hard

In a galvanic cell, the cathode metal increases in mass by

0.635\text{ g}

(Cu). How many coulombs flowed? (

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

F=96500\text{ C/mol}

)

Example 11

medium

An electrochemical cell uses

Sn^{2+}/Sn

(

-0.14\text{ V}

) and

Cu^{2+}/Cu

(

+0.34\text{ V}

). Identify the anode, cathode, electron flow, and

E^\circ_{cell}

Example 12

easy

Which electrode in a galvanic cell is labeled with the negative terminal: anode or cathode?

Example 13

medium

For an electrochemical cell with

E^\circ_{cell} = +0.46\text{ V}

and

n = 2

, compute

\Delta G^\circ

in kJ. (

F = 96500\text{ C/mol}

)

Example 14

hard

An electrochemical cell uses

Cr^{3+}/Cr

(

-0.74\text{ V}

) and

Fe^{2+}/Fe

(

-0.44\text{ V}

). Determine the spontaneous direction and find

E^\circ_{cell}

Example 15

medium

Fill in the blank: at the anode, the electrode material in a

Zn|Zn^{2+}

half-cell ____ over time.

Example 16

medium

A cell pairs

Zn \rightarrow Zn^{2+} + 2e^-

and

Cu^{2+} + 2e^- \rightarrow Cu

. Write the overall reaction.

Example 17

hard

A student claims that in a galvanic cell, electrons travel through the salt bridge to complete the circuit. Identify the error and give the correction.

Example 18

easy

Why does an electrochemical cell separate the two half-reactions?

Example 19

hard

An electrolytic cell electrolyzes molten

AlCl_3

. Find the mass of Al produced by

9650\text{ C}

of charge. (

M(Al)=27\text{ g/mol}

F=96500\text{ C/mol}

)

Example 20

medium

In an electrochemical cell, the salt bridge contains

KNO_3

. Which ion moves toward the cathode?

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Related Concepts

Electrochemistry Electrolytic Cell