#cell reaction

Variation of Conductivity with Concentration and Measurement

What is the emf of a cell with the reaction Mg(s) + 2Ag⁺(aq) → Mg²⁺(aq) + 2Ag(s) at standard conditions, given E°Mg²⁺/Mg

E°cell = E°cathode - E°anode = 0.80 - (-2.36) = 3.16 V .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Variation of Conductivity with Concentration and Measurement

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Nernst Equation and Gibbs Energy and Equilibrium Constant

The standard Gibbs energy change for a cell reaction is -212.27 kJ/mol, and 2 electrons are transferred. What is the sta

Δr G° = -n F E°cell . -212270 = -2 × 96500 × E°cell , E°cell = 1.1 V .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Electrolytic Cells and Electrolysis and Faraday's Laws

What is the equilibrium constant for a cell reaction with E°cell = 0.354 V at 298 K involving 2 electrons?

E°cell = (0.059/n) log Kc , 0.354 = (0.059/2) log Kc , log Kc = 12, Kc = 10¹² .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrolytic Cells and Electrolysis and Faraday's Laws

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Electrolytic Cells and Electrolysis and Faraday's Laws

What is the equilibrium constant for a cell reaction with E°cell = 0.118 V at 298 K involving 1 electron?

E°cell = (0.059/n) log Kc , 0.118 = 0.059 log Kc , log Kc = 2, Kc = 10² .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrolytic Cells and Electrolysis and Faraday's Laws

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Electrochemical Cells - Galvanic Cells and Electrode Potential

What is the standard emf of a cell with the reaction Co(s) + 2Ag⁺(aq) → Co²⁺(aq) + 2Ag(s) ? (Given: E°Co²⁺/Co = -0.28 V

E°cell = E°cathode - E°anode = 0.80 - (-0.28) = 1.08 V .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential

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Electrochemical Cells - Galvanic Cells and Electrode Potential

What is the standard emf of a cell with the reaction Cr(s) + 3Ag⁺(aq) → Cr³⁺(aq) + 3Ag(s) ? (Given: E°Cr³⁺/Cr = -0.74 V

E°cell = E°cathode - E°anode = 0.80 - (-0.74) = 1.54 V .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential

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Electrochemical Cells - Galvanic Cells and Electrode Potential

A cell reaction has Δr G° = -212300 J/mol and involves 2 electrons at 298 K. What is the equilibrium constant?

Δr G° = -n F E°cell , E°cell = (212300/2 × 96500) = 1.10 V . E°cell = (0.059/n) log Kc , 1.10 = (0.059/2) log Kc , log Kc = 37.29, Kc ≈ 10³⁷ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential

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Electrochemical Cells - Galvanic Cells and Electrode Potential

A cell reaction has Δr G° = -212300 J/mol and involves 2 electrons at 298 K. What is the equilibrium constant?

Δr G° = -n F E°cell , E°cell = (212300/2 × 96500) = 1.10 V . E°cell = (0.059/n) log Kc , 1.10 = (0.059/2) log Kc , log Kc = 37.29, Kc ≈ 10³⁷ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential

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Corrosion and Applications of Electrochemistry

What is the standard emf of a cell with the reaction Sn(s) + Pb²⁺(aq) → Sn²⁺(aq) + Pb(s) ? (Given: E°Sn²⁺/Sn = -0.14 V ,

E°cell = E°cathode - E°anode = -0.13 - (-0.14) = 0.01 V .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry

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Corrosion and Applications of Electrochemistry

What is the standard emf of a cell with the reaction Sn(s) + Pb²⁺(aq) → Sn²⁺(aq) + Pb(s) ? (Given: E°Sn²⁺/Sn = -0.14 V ,

E°cell = E°cathode - E°anode = -0.13 - (-0.14) = 0.01 V .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry

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Corrosion and Applications of Electrochemistry

What is the equilibrium constant for a cell reaction with E°cell = 0.46 V at 298 K involving 2 electrons?

E°cell = (0.059/n) log Kc . 0.46 = (0.059/2) log Kc , log Kc = 15.59 , Kc ≈ 3.9 × 10¹⁵ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry

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Corrosion and Applications of Electrochemistry

In a mercury cell, what is the overall cell reaction?

Anode: Zn + 2OH⁻ → ZnO + H₂O + 2e⁻ . Cathode: HgO + H₂O + 2e⁻ → Hg + 2OH⁻ . Overall: Zn + HgO → ZnO + Hg .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Corrosion and Applications of Electrochemistry

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