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 cell notation for the redox reaction given below
3 Cl2(g) + 2 Fe(s) → 6 Cl − (aq) + 2 Fe3+(aq)
A) Fe(s) | Fe3+(aq) || Cl2(g), Cl −(aq) | Pt
B) Cl − (aq) | Cl2(g) | Pt || Fe3+(aq)

Determine the cell notation for the redox reaction given below

3 Cl_{2}(*g*) + 2 Fe(*s*) → 6 Cl ^{−} (*aq*) + 2 Fe^{3+}(*aq*)

A) Fe(*s*) | Fe^{3+}(*aq*) || Cl_{2}(*g*), Cl ^{−}(*aq*) | Pt

B) Cl ^{−} (*aq*) | Cl_{2}(*g*) | Pt || Fe^{3+}(*aq*) | Fe(*s*)

C) Fe(*s*) | Fe^{3+}(*aq*) || Cl_{2}(*g*) | Cl ^{−} (*aq*) | Pt

D) Fe(*s*) | Cl_{2}(*g*) || Fe^{3+}(*aq*) | Cl ^{−} (*aq*) | Pt

E) Pt | Cl_{2}(*g*) | Cl ^{−} (*aq*) || Fe^{3+}(*aq*) | Fe(*s*)

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