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Anode: Zn(Hg) + 2OH⁻ → ZnO(s) + H₂O + 2e⁻ . Product is ZnO.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
Zn + 2OH⁻ → ZnO + H₂O + 2e⁻ . 1 mol Zn (68 g) requires 2F. Moles = (0.68/68) = 0.01 mol , Charge = 0.01 × 2 = 0.02 F .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
Reaction: Zn(Hg) + HgO(s) → ZnO(s) + Hg(l) . Zn is oxidized, so it’s the reducing agent.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry
Reaction: Zn(Hg) + HgO(s) → ZnO(s) + Hg(l) . Zn is oxidized, so it’s the reducing agent.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry
The anode in a lead storage battery is lead (Pb).
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Batteries - Primary Secondary and Fuel Cells
Charging anode: PbSO₄ + 2e⁻ → Pb + SO₄²⁻ . Pb has oxidation state 0.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Batteries - Primary Secondary and Fuel Cells
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