14 public questions tagged with this topic.
Mass of C = (12/44) × 0.66 = 0.18 g. Mass of H = (2/18) × 0.135 = 0.015 g. Ratio C:H = (0.18/12)/(0.015/1) = 1:1. Empirical formula = CH.
Ref: NCERT Class 11 Chemistry > Chapter 8: Organic Chemistry - Some Basic Principles and Techniques > Topic: Electronic Effects - Inductive Mesomeric Hyperconjugation and Resonance
For 100 g: C = 40 g, H = 6.67 g, O = 53.33 g. Moles: C ≈ 3.33, H ≈ 6.67, O ≈ 3.33. Ratio = 1 : 2 : 1; empirical formula = CH₂O, mass = 30 g/mol. n = 180/30 = 6; molecular formula = C₆H₁₂O₆.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
Mass of C = (12/44) × 1.76 ≈ 0.48 g; mass of H = (2/18) × 0.72 = 0.08 g. Total = 0.56 g (matches). Moles: C = 0.48/12 = 0.04, H = 0.08/1 = 0.08; ratio = 1 : 2; empirical formula = CH₂, mass = 14 g/mol. n = 56/14 = 4; molecular formula = C₄H₈.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
Moles = 2.5/22.4 ≈ 0.1116 mol; molar mass = 5/0.1116 ≈ 44.8 g/mol. Assume NₓOᵧ: 14x + 16y = 44.8. Simplest ratio: N₂O (14×2 + 16 = 44); empirical formula = N₂O.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
For 100 g: C = 36.36 g, H = 6.06 g, O = 57.58 g. Moles: C ≈ 3.03, H ≈ 6.06, O ≈ 3.6. Ratio ≈ 1 : 2 : 1; empirical formula = CH₂O.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Dalton's Atomic Theory and Atomic and Molecular Masses
For 100 g: Na = 32.43 g, S = 22.52 g, O = 45.05 g. Moles: Na ≈ 1.41, S ≈ 0.704, O ≈ 2.82. Ratio = 2 : 1 : 4; empirical formula = Na₂SO₄.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Dalton's Atomic Theory and Atomic and Molecular Masses
For 100 g: C = 26.67 g, H = 2.22 g, O = 71.11 g. Moles: C ≈ 2.22, H = 2.22, O ≈ 4.44. Ratio = 1 : 1 : 2; empirical formula = CHO₂.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Dalton's Atomic Theory and Atomic and Molecular Masses
For 100 g: C = 40 g, H = 6.67 g, O = 53.33 g. Moles: C ≈ 3.33, H ≈ 6.67, O ≈ 3.33. Ratio = 1 : 2 : 1; empirical formula = CH₂O.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Dalton's Atomic Theory and Atomic and Molecular Masses
For 100 g: Mg = 24 g, S = 28 g, O = 48 g. Moles: Mg = 1, S = 0.875, O = 3. Ratio ≈ 1 : 1 : 3 (adjusted); empirical formula = MgSO₃.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Dalton's Atomic Theory and Atomic and Molecular Masses
For 100 g: C = 38.71 g, H = 9.68 g, O = 51.61 g. Moles: C ≈ 3.23, H ≈ 9.68, O ≈ 3.23. Ratio = 1 : 3 : 1; empirical formula = CH₃O.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Dalton's Atomic Theory and Atomic and Molecular Masses
For 100 g: C = 52.17 g, H = 13.04 g, O = 34.78 g. Moles: C ≈ 4.35, H ≈ 13.04, O ≈ 2.17. Divide by smallest (2.17): C ≈ 2.00, H ≈ 6.00, O = 1.00. Ratio = 2:6:1; empirical formula = C₂H₆O.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Dalton's Atomic Theory and Atomic and Molecular Masses
For 100 g: C = 52.17 g, H = 13.04 g, O = 34.78 g. Moles: C ≈ 4.35, H ≈ 13.04, O ≈ 2.17. Ratio = 2 : 6 : 1; empirical formula = C₂H₆O.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Dalton's Atomic Theory and Atomic and Molecular Masses
