11 public questions tagged with this topic.
The dry cell (Leclanché cell) has a potential of approximately 1.5 V.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
Charge = 0.1 × 19300 = 1930 C . Cathode: MnO₂ + H⁺ + e⁻ → MnO(OH) , 1 mol MnO₂ requires 1F. Faradays = (1930/96500) = 0.02 F , Moles = 0.02 mol , Mass = 0.02 × 87 = 1.74 g .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrolytic Cells and Electrolysis and Faraday's Laws
Charge = 0.25 × 9650 = 2412.5 C . Zn → Zn²⁺ + 2e⁻ , 1 mol Zn (65 g) requires 2F. Faradays = (2412.5/96500) = 0.025 F , Moles = (0.025/2) = 0.0125 mol , Mass = 0.0125 × 65 = 0.8125 g .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrolytic Cells and Electrolysis and Faraday's Laws
Anode: Zn → Zn²⁺ + 2e⁻ . Zn is oxidized, so it’s the reducing agent.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
Cathode: MnO₂ + NH₄⁺ + e⁻ → MnO(OH) + NH₃ . In MnO₂ , Mn = +4; in MnO(OH) , Mn + 2(-2) + 1 = 0, Mn = +3.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry
Cathode: MnO₂ + NH₄⁺ + e⁻ → MnO(OH) + NH₃ . In MnO₂ , Mn = +4; in MnO(OH) , Mn + 2(-2) + 1 = 0, Mn = +3.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry
MnO₂ + H⁺ + e⁻ → MnO(OH) . Moles = (0.435/87) = 0.005 mol , Charge = 0.005 × 96500 = 482.5 C .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Batteries - Primary Secondary and Fuel Cells
MnO₂ + H⁺ + e⁻ → MnO(OH) . Moles = (0.435/87) = 0.005 mol , Charge = 0.005 × 96500 = 482.5 C .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Batteries - Primary Secondary and Fuel Cells
The electrolyte in a dry cell is a moist paste of NH₄Cl and ZnCl₂.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Batteries - Primary Secondary and Fuel Cells
MnO₂ + H⁺ + e⁻ → MnO(OH) . Molar mass = 55 + 32 = 87 g/mol . Moles = (0.87/87) = 0.01 mol , Charge = 0.01 × 96500 = 965 C .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Batteries - Primary Secondary and Fuel Cells
In a dry cell, the cathode is a graphite rod surrounded by MnO₂.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Batteries - Primary Secondary and Fuel Cells
