Subjects

Sections | |||
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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 | 85 mins | 0 completed | Learn |

Batteries and Electricity | 9 mins | 0 completed | Learn |

Additional Practice |
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Cell Notation |

Standard Hydrogen Electrode |

Cell Potential |

Electroplating |

Electrolysis of Water & Mixture of Ions |

Additional Guides |
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Nernst Equation |

Solution: Determine the redox reaction represented by the following cell notation.
Fe(s) | Fe2+(aq) ‖ Cu2+(aq) | Cu(s)
a) Cu(s) + Fe2+(aq) → Fe(s) + Cu 2+(aq)
b) Fe(s) + Cu2+(aq) → Cu(s) + Fe 2+(aq)
c) 2

Determine the redox reaction represented by the following cell notation.

Fe(s) | Fe^{2+}(aq) ‖ Cu^{2+}(aq) | Cu(s)

a) Cu(s) + Fe^{2+}(aq) → Fe(s) + Cu ^{2+}(aq)

b) Fe(s) + Cu^{2+}(aq) → Cu(s) + Fe ^{2+}(aq)

c) 2 Fe(s) + Cu2+(aq) → Cu(s) + 2 Fe ^{2+}(aq)

d) 2 Cu(s) + Fe^{2+}(aq) → Fe(s) + 2 Cu ^{2+}(aq)

e) 3 Fe(s) + 2 Cu^{2+}(aq) → 2 Cu(s) + 3 Fe ^{2+}(aq)

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