#standard emf

Variation of Conductivity with Concentration and Measurement

What is the standard emf of a cell with the reaction Co(s) + Ni²⁺(aq) → Co²⁺(aq) + Ni(s) ? (Given: E°Co²⁺/Co = -0.28 V ,

E°cell = E°cathode - E°anode = -0.25 - (-0.28) = 0.03 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

A cell has E°cell = 0.88 V and Δr G° = -169840 J/mol at 298 K. How many electrons are transferred? (F = 96500 C/mol)

Δr G° = -n F E°cell , -169840 = -n × 96500 × 0.88 . n = (169840/96500 × 0.88) = (169840/84920) ≈ 2 .

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

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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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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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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 standard emf of a cell with the reaction 2Al(s) + 3Cd²⁺(aq) → 2Al³⁺(aq) + 3Cd(s) ? (Given: E°Al³⁺/Al = -1.66

E°cell = E°cathode - E°anode = -0.40 - (-1.66) = 1.26 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 2Al(s) + 3Cd²⁺(aq) → 2Al³⁺(aq) + 3Cd(s) ? (Given: E°Al³⁺/Al = -1.66

E°cell = E°cathode - E°anode = -0.40 - (-1.66) = 1.26 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 Pb(s) + Hg₂²⁺(aq) → Pb²⁺(aq) + 2Hg(l) ? (Given: E°Pb²⁺/Pb = -0.13 V

E°cell = E°cathode - E°anode = 0.79 - (-0.13) = 0.92 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 Pb(s) + Hg₂²⁺(aq) → Pb²⁺(aq) + 2Hg(l) ? (Given: E°Pb²⁺/Pb = -0.13 V

E°cell = E°cathode - E°anode = 0.79 - (-0.13) = 0.92 V .

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

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