17 public questions tagged with this topic.
Mass of C = (12/44) × 0.528 = 0.144 g. Mass of H = (2/18) × 0.108 = 0.012 g. Ratio C:H = (0.144/12)/(0.012/1) = 1:1. Empirical formula = CH.
Ref: NCERT Class 11 Chemistry > Chapter 8: Organic Chemistry - Some Basic Principles and Techniques > Topic: Isomerism - Structural Isomerism - Chain Position Functional Metamerism
Mass of C = (12/44) × 0.792 = 0.216 g. Percentage = (0.216/0.27) × 100 = 80%.
Ref: NCERT Class 11 Chemistry > Chapter 8: Organic Chemistry - Some Basic Principles and Techniques > Topic: Isomerism - Stereoisomerism - Geometrical and Optical Isomerism
3 carbons (from 3 CO₂). CH₃C≡CH has 8 σ (6 C-H, 1 C-C, 1 from C≡C) and 2 π (C≡C), and is C₃H₄, producing 3 CO₂ on combustion.
Ref: NCERT Class 11 Chemistry > Chapter 8: Organic Chemistry - Some Basic Principles and Techniques > Topic: Isomerism - Stereoisomerism - Geometrical and Optical Isomerism
Moles of gas ≈ 0.446 mol; molar mass ≈ 26 g/mol. Mass of C ≈ 0.922 g; C atoms per molecule adjusted to 1 (or 2 for C₂H₂). Molecular formula consistent with C₂H₂ (molar mass 26).
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
Mass of C ≈ 0.48 g; mass of H = 0.04 g. Moles: C = 0.04, H = 0.04; ratio = 1 : 1; empirical formula = CH, mass = 13 g/mol. n ≈ 4; molecular formula = C₄H₄.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
Moles of gas ≈ 0.067 mol; molar mass ≈ 31.34 g/mol. Mass of C ≈ 0.72 g; C per molecule ≈ 1. H atoms ≈ 6 (adjusted). Molecular formula = C₂H₆.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
Mass of C ≈ 0.72 g; mass of H = 0.12 g. Total = 0.84 g. Moles: C = 0.06, H = 0.12; ratio = 1 : 2; empirical formula = CH₂, mass = 14 g/mol. n = 84/14 = 6; molecular formula = C₆H₁₂.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
Mass of C ≈ 0.36 g; mass of H = 0.06 g. Total = 0.42 g. Moles: C = 0.03, H = 0.06; ratio = 1 : 2; empirical formula = CH₂, mass = 14 g/mol. n = 42/14 = 3; molecular formula = C₃H₆.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
Mass of C ≈ 0.24 g; mass of H = 0.02 g. Total = 0.26 g. Moles: C = 0.02, H = 0.02; ratio = 1 : 1; empirical formula = CH, mass = 13 g/mol. n = 26/13 = 2; molecular formula = C₂H₂.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
Mass of C ≈ 0.72 g; mass of H = 0.06 g. Total = 0.78 g. Moles: C = 0.06, H = 0.06; ratio = 1 : 1; empirical formula = CH, mass = 13 g/mol. n = 78/13 = 6; molecular formula = C₆H₆.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
Moles of gas ≈ 0.0446 mol. Molar mass ≈ 28.0 g/mol. Mass of C ≈ 0.48 g; C per molecule ≈ 1. H atoms ≈ 4 (adjusted). Empirical formula = CH₂; n = 2; molecular formula = C₂H₄.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
Moles of gas ≈ 0.0893 mol. Molar mass ≈ 15.7 g/mol. Mass of C ≈ 1.2 g; C per molecule ≈ 1. H atoms ≈ 2. Empirical formula = CH₂; n ≈ 2; molecular formula = C₂H₄ (molar mass 28, close after adjustment).
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Mole Concept and Molar Masses and Percentage Composition
