12 public questions tagged with this topic.
Positive E° indicates Cu cannot displace H 2 from acids, as it is less reactive than hydrogen.
Ref: NCERT Class 12 Chemistry > Chapter 4: d and f Block Elements > Topic: Applications of d and f Block Elements
E°cell = 0.00 - (-0.76) = 0.76 V . Ecell = 0.76 - (0.059/2) log (0.001/1²) = 0.76 + 0.0885 = 0.8485 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Variation of Conductivity with Concentration and Measurement
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
E°cell = 0.00 - (-1.18) = 1.18 V . Ecell = 1.18 - (0.059/2) log (0.05/0.005²) = 1.18 - 0.07375 = 1.10625 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
E°cell = 1.07 - (-0.76) = 1.83 V . Ecell = 1.83 - (0.059/2) log ([Zn²⁺][Br⁻]²/1) = 1.83 - 0.0295 log (0.001 × 0.000004) = 1.83 + 0.148 = 1.978 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
E = E° - (0.059/n) log (1/[H⁺]) , [H⁺] = 10⁻⁷ , n = 1 . E = 0 - 0.059 × 7 = -0.413 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
E = E° - (0.059/n) log (1/[H⁺]) , [H⁺] = 10⁻⁷ , n = 1 . E = 0 - 0.059 × 7 = -0.413 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
E°cell = -0.25 - (-0.40) = 0.15 V . Ecell = 0.15 - (0.059/2) log (0.01/0.1) = 0.15 + 0.0295 = 0.1795 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry
E°cell = (0.059/n) log Kc , 0.295 = 0.059 log Kc , log Kc = 5, Kc = 10⁵ .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry
E°cell = (0.059/n) log Kc , 0.295 = 0.059 log Kc , log Kc = 5, Kc = 10⁵ .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry
E°cell = 0.80 - (-0.13) = 0.93 V . Ecell = 0.93 - (0.059/2) log (0.005/0.05²) = 0.93 - 0.0295 = 0.9005 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry
