Electrochemical Cell (Galvanic) – AP Chemistry | ShowMeClass

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Galvanic (Voltaic) Cell

AP Chemistry · Unit 9: Electrochemistry

Learning Objectives

Identify anode (oxidation) and cathode (reduction)

Trace electron flow through external circuit

Explain salt bridge function

Calculate cell potential E°cell using standard reduction potentials

Apply the Nernst equation for non-standard conditions

Key Equations

Cell Notation

Remember

Anode = Oxidation (loses e⁻, mass decreases)
Cathode = Reduction (gains e⁻, mass increases)
Mnemonic: AN OX & RED CAT
Electrons flow: anode → wire → cathode
Salt bridge ions balance charge

Galvanic CellElectrochemistryAP ChemistryUnit 9

E°cell—

E (Nernst)—

ΔG°—

Spontaneous—

Cell Pair

[Anode ion] (M) 1.00

[Cathode ion] (M) 1.00

Temperature (K) 298

Display

Cell Analysis

📝 Quick Quiz▼

1. In a galvanic cell, oxidation occurs at the:

Cathode Anode Salt bridge Wire

2. For Zn-Cu cell, E°cell is approximately:

+0.34 V −1.10 V +1.10 V +0.76 V

3. A positive E°cell means the reaction is:

Non-spontaneous At equilibrium Spontaneous Endothermic