Subjects
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Redox Reaction | 32 mins | 0 completed | Learn Summary |
Balancing Redox Reaction | 31 mins | 0 completed | Learn |
The Nernst Equation | 11 mins | 0 completed | Learn |
Faraday's Constant | 10 mins | 0 completed | Learn |
Galvanic Cell | 90 mins | 0 completed | Learn |
Batteries and Electricity | 9 mins | 0 completed | Learn |
Additional Practice |
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Cell Notation |
Standard Hydrogen Electrode |
Ion Selective Electrodes |
Cell Potential |
Electroplating |
Electrolysis of Water & Mixture of Ions |
Additional Guides |
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Nernst Equation (IGNORE) |
Batteries act as spontaneous electrochemical cells that help to generate electricity.
These types of batteries get their names from the fact that they contain very little water.
The overall reaction within a typical dry-cell battery is
Zn (s) + 2 MnO2 (s) + 2 NH4+ (aq) → Zn2+ (aq) + Mn2O3 (s) + 2 NH3 (g) + H2O (l)
These types of batteries get their names from the fact that they operate within a basic medium.
Concept #2: The counterpart to an acidic dry-cell battery is the alkaline battery.
The overall reaction within a typical alkaline battery is
Zn (s) + 2 MnO2 (s) + 2 H2O (l) → Zn(OH)2 (s) + 2 MnO(OH) (s)
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