77 public questions tagged with this topic.
Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O . 6 electrons per mole.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Variation of Conductivity with Concentration and Measurement
2IO₃⁻ + 12H⁺ + 10e⁻ → I₂ + 6H₂O . For 1 mol IO₃⁻ , 5 electrons.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
The cell reaction is Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s) . E°cell = E°cathode - E°anode = 0.34 - (-0.76) = 1.10 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
E°cell = (0.059/n) log Kc , 1.36 = (0.059/n) × 46 , n = (2.714/1.36) ≈ 2 .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
E°cell = (0.059/n) log Kc , 1.36 = (0.059/n) × 46 , n = (2.714/1.36) ≈ 2 .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
NO₃⁻ + 10H⁺ + 8e⁻ → NH₄⁺ + 3H₂O . 8 electrons per mole.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
MnO₄⁻ + 2H₂O + 3e⁻ → MnO₂ + 4OH⁻ . 3 electrons per mole.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential
ClO₄⁻ + 8H⁺ + 8e⁻ → Cl⁻ + 4H₂O . 8 electrons per mole.
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Conductance - Conductivity Molar Conductivity and Kohlrausch Law
F (0 in F₂) becomes -1 in SF₄ and HF, gaining electrons; S (-2 to +4) is oxidized.
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Types of Redox Reactions - Combination Decomposition Displacement
HNO₃ (N: +5) is reduced to NO (N: +2), oxidizing Sn (0 to +4).
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Types of Redox Reactions - Combination Decomposition Displacement
In C + O₂ → CO₂, C (0) is oxidized to +4, and O₂ (0) is reduced to -2, making it a redox combination reaction.
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Types of Redox Reactions - Combination Decomposition Displacement
In 2Ag₂O → 4Ag + O₂, Ag (+1) is reduced to 0, and O (-2) is oxidized to 0.
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Types of Redox Reactions - Combination Decomposition Displacement
