Redox Reactions and Electrochemistry: One-Page Formula Sheet

Redox Reactions and Electrochemistry — formula sheet

Formulas

• E_cell = E°_cathode − E°_anode
• Nernst: E = E° − (0.059/n) log Q at 298 K
• ΔG° = −nFE°
• Faraday: m = (M/nF) × I × t

Key ideas

• Oxidation is loss of electrons; occurs at the anode
• Higher reduction potential means stronger oxidising agent
• Kohlrausch's law gives Λ° of weak electrolytes
• Faraday's laws relate charge and mass deposited

Traps to avoid

• Reversing cathode and anode potentials
• Wrong n in the Nernst equation
• Forgetting molar conductivity rises on dilution

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