Electrochemistry

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Electrochemistry is the study of the relationship between chemical reactions and electrical energy. Its two main applications are: (1) Production of electricity from spontaneous chemical reactions (ga

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A galvanic cell converts chemical energy of a spontaneous redox reaction into electrical energy. Example: Daniell cell with Zn and Cu electrodes. Cell reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s). Ce

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In a galvanic cell: Anode is the electrode where oxidation occurs (negative terminal, electrons are released). Cathode is the electrode where reduction occurs (positive terminal, electrons are consume

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Standard electrode potential (E°) is the potential of an electrode when all species are at unit concentration (1 M) at 298 K and 1 bar pressure. It is measured relative to Standard Hydrogen Electrode

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Nernst equation: E = E° - (RT/nF) ln(1/[Mⁿ⁺]) = E° - (0.059/n) log(1/[Mⁿ⁺]) at 298 K. Significance: It relates electrode potential to concentration of ions. Shows that potential decreases as concentra

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E_cell = E°_cell - (RT/2F) ln([Zn²⁺]/[Cu²⁺]) = E°_cell - (0.059/2) log([Zn²⁺]/[Cu²⁺]) at 298 K. Where E°_cell = E°_Cu²⁺/Cu - E°_Zn²⁺/Zn = 0.34 - (-0.76) = 1.10 V.

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ΔrG = -nFE_cell. For standard conditions: ΔrG° = -nFE°_cell. Significance: Negative ΔrG means spontaneous reaction (positive E_cell). This relationship connects thermodynamics with electrochemistry an

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Conductivity (κ) = 1/ρ = conductance of 1 m³ solution between electrodes 1 m apart. Units: S m⁻¹ or S cm⁻¹. Molar conductivity (Λm) = κ/c = conductivity per unit concentration. Units: S m² mol⁻¹ or S