Corrosion and Applications of Electrochemistry

Corrosion and Applications of Electrochemistry

In a dry cell, what is the oxidation state of manganese in the cathode product MnO(OH)?

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

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Corrosion and Applications of Electrochemistry

In a dry cell, what is the oxidation state of manganese in the cathode product MnO(OH)?

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

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Corrosion and Applications of Electrochemistry

The degree of dissociation of a weak electrolyte is 0.05, and its molar conductivity is 19 S cm² mol⁻¹. What is its Lamb

α = (Lambdam/Lambdam°) , 0.05 = (19/Lambdam°) , Lambdam° = 380 S cm² mol⁻¹ .

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

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Corrosion and Applications of Electrochemistry

The degree of dissociation of a weak electrolyte is 0.05, and its molar conductivity is 19 S cm² mol⁻¹. What is its Lamb

α = (Lambdam/Lambdam°) , 0.05 = (19/Lambdam°) , Lambdam° = 380 S cm² mol⁻¹ .

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 Gibbs energy change for a cell with E°cell = 1.05 V and 2 electrons transferred? (F = 96500 C/mol)

Δr G° = -n F E°cell = -2 × 96500 × 1.05 = -202650 J/mol = -202.65 kJ/mol .

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 Gibbs energy change for a cell with E°cell = 1.05 V and 2 electrons transferred? (F = 96500 C/mol)

Δr G° = -n F E°cell = -2 × 96500 × 1.05 = -202650 J/mol = -202.65 kJ/mol .

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

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Corrosion and Applications of Electrochemistry

In the electrolysis of molten NaCl, what is the product at the cathode?

Cathode: Na⁺ + e⁻ → Na . Sodium metal is produced.

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

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Corrosion and Applications of Electrochemistry

In the electrolysis of molten NaCl, what is the product at the cathode?

Cathode: Na⁺ + e⁻ → Na . Sodium metal is produced.

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 emf of the cell Cd(s) | Cd²⁺(0.01 M) || Ni²⁺(0.1 M) | Ni(s) at 298 K? (Given: E°Cd²⁺/Cd = -0.40 V , E°Ni²⁺/N

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

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Corrosion and Applications of Electrochemistry

What is the emf of the cell Cd(s) | Cd²⁺(0.01 M) || Ni²⁺(0.1 M) | Ni(s) at 298 K? (Given: E°Cd²⁺/Cd = -0.40 V , E°Ni²⁺/N

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

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Corrosion and Applications of Electrochemistry

In a mercury cell, what is the reducing agent?

Reaction: Zn(Hg) + HgO(s) → ZnO(s) + Hg(l) . Zn is oxidized, so it’s the reducing agent.

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 reducing agent?

Reaction: Zn(Hg) + HgO(s) → ZnO(s) + Hg(l) . Zn is oxidized, so it’s the reducing agent.

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

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