7 public questions tagged with this topic.
w = -nRT ln(P₁/P₂) = -1 × 8.314 × 300 × ln(5/1) = -2494.2 × 1.609 = -4013 J.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Third Law of Thermodynamics and Applications
Moles = 2.24/22.4 = 0.1 mol. Molar mass = 3.2/0.1 = 32 g/mol.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Stoichiometry and Stoichiometric Calculations and Limiting Reagent
Moles = 5.6/22.4 = 0.25 mol. Molar mass = 8/0.25 = 32 g/mol.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Stoichiometry and Stoichiometric Calculations and Limiting Reagent
Moles = 11.2/22.4 = 0.5 mol. Molar mass = 16/0.5 = 32 g/mol.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Stoichiometry and Stoichiometric Calculations and Limiting Reagent
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 = 4.48/22.4 = 0.2 mol. Molar mass = 2/0.2 = 10 g/mol.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Laws of Chemical Combination - Conservation Mass Definite Multiple
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
