6 public questions tagged with this topic.
E°cell = 1.36 - 0.34 = 1.02 V . Ecell = 1.02 - (0.059/2) log ([Cu²⁺][Cl⁻]²/PCl_₂) = 1.02 - 0.0295 log (0.01 × 0.0025/0.5) = 1.02 + 0.053 = 1.073 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
E°cell = 0.00 - (-0.14) = 0.14 V . Ecell = 0.14 - (0.059/2) log (0.05/0.1²) = 0.14 + 0.039 = 0.179 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
E°cell = 0.00 - (-0.28) = 0.28 V . Ecell = 0.28 - (0.059/2) log (0.02/0.01²) = 0.28 - 0.07375 = 0.20625 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
E°cell = 1.07 - (-0.40) = 1.47 V . Ecell = 1.47 - (0.059/2) log ([Cd²⁺][Br⁻]²/1) = 1.47 - 0.0295 log (0.005 × 0.0001) = 1.47 + 0.103 = 1.573 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
E°cell = 0.80 - (-0.74) = 1.54 V . Ecell = 1.54 - (0.059/3) log ([Cr³⁺]/[Ag⁺]³) = 1.54 - 0.01967 log (0.002/0.000125) = 1.54 - 0.025 = 1.515 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
E°cell = 1.07 - (-0.28) = 1.35 V . Ecell = 1.35 - (0.059/2) log ([Co²⁺][Br⁻]²/1) = 1.35 - 0.0295 log (0.01 × 0.0025) = 1.35 + 0.073 = 1.423 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
