#ethanol combustion

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Enthalpy Changes - Reaction Formation Combustion and Hess's Law

Calculate Δ H for C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l) using: Δ Hf° (C₂H₅OH,l) = -277.7 kJ/mol, Δ Hf° (CO₂,g) = -393.5

Δ H = [2(-393.5) + 3(-285.8)] - [-277.7 + 3(0)] = -787 - 857.4 + 277.7 = -1366.7 kJ/mol.

Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Enthalpy Changes - Reaction Formation Combustion and Hess's Law

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Importance and Nature of Chemistry and Properties of Matter

What volume of O₂ at STP is required to burn 5 g of C₂H₅OH completely to CO₂ and H₂O? (Molar mass: C₂H₅OH = 46 g/mol)

Reaction: C₂H₅OH + 3O₂ → 2CO₂ + 3H₂O. Moles of C₂H₅OH = 5/46 ≈ 0.1087 mol. 1 mol needs 3 mol O₂; 0.1087 mol needs 0.3261 mol. Volume = 0.3261 × 22.4 ≈ 7.3 L.

Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Importance and Nature of Chemistry and Properties of Matter

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#ethanol combustion

No questions with this tag

Calculate Δ H for C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l) using: Δ Hf° (C₂H₅OH,l) = -277.7 kJ/mol, Δ Hf° (CO₂,g) = -393.5

What volume of O₂ at STP is required to burn 5 g of C₂H₅OH completely to CO₂ and H₂O? (Molar mass: C₂H₅OH = 46 g/mol)

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