6 public questions tagged with this topic.
Ecell = E°cell - (0.059/n) log ([Ox]/[Red]) , 0.68 = 0.62 - (0.059/n) log (0.01/0.1) . 0.06 = (0.059/n) × 1 , n = (0.059/0.06) ≈ 1 .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
E°cell = 1.36 - (-0.25) = 1.61 V . Ecell = 1.61 - (0.059/2) log ([Ni²⁺][Cl⁻]²/PCl_₂) = 1.61 - 0.0295 log (0.001 × 0.01/2) = 1.61 + 0.103 = 1.713 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
E°cell = 0.80 - 0.34 = 0.46 V . Ecell = 0.46 - (0.059/2) log (0.01/0.1²) = 0.46 + 0.0295 = 0.4895 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
Reaction: Fe(s) + 2Ag⁺(aq) → Fe²⁺(aq) + 2Ag(s) . E°cell = E°cathode - E°anode = 0.80 - (-0.44) = 1.24 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
The cell reaction is Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s) . E°cell = E°cathode - E°anode = 0.34 - (-0.76) = 1.10 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
E°cell = 0.34 - (-0.44) = 0.78 V . Ecell = 0.78 - (0.059/2) log (0.001/0.1) = 0.78 + 0.059 = 0.839 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
