6 public questions tagged with this topic.
Cathode: 2H₂O + 2e⁻ → H₂ + 2OH⁻ , Anode: 2H₂O → O₂ + 4H⁺ + 4e⁻ . Total moles = (0.336/22.4) = 0.015 mol (H₂:O₂ = 2:1), H₂ = 0.01 mol, O₂ = 0.005 mol. Charge = (0.01 × 2 + 0.005 × 4) × 96500 = 0.04 × 96500 = 3860 C .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrolytic Cells and Electrolysis and Faraday's Laws
Moles = 5.6/22.4 = 0.25 mol. Molar mass = 2/0.25 = 8 g/mol.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Reactions in Solutions and Mass Percentage and Numericals
Moles = 1.12/22.4 = 0.05 mol. Molar mass = 1.6/0.05 = 32 g/mol.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Reactions in Solutions and Mass Percentage and Numericals
Moles = 1.12/22.4 = 0.05 mol. Molar mass = 1.4/0.05 = 28 g/mol.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Reactions in Solutions and Mass Percentage and Numericals
Moles = 0.56/22.4 = 0.025 mol. Molar mass = 0.64/0.025 = 25.6 g/mol.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Reactions in Solutions and Mass Percentage and Numericals
Moles = 3.36/22.4 = 0.15 mol. Molar mass = 4.8/0.15 = 32 g/mol.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Importance and Nature of Chemistry and Properties of Matter
