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#methane combustion

6 public questions tagged with this topic.

Thermodynamic Terms - System Surroundings and Types of Systems

For the reaction CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l) , Δ H = -890.00 kJ/mol at 298 K. What is Δ U ? ( R = 8.314 J/mol·K )

For Δ ng = 1 - 3 = -2 , RT = 8.314 × 298 × 10⁻³ = 2.4776 kJ . Using Δ H = Δ U + Δ ng RT , Δ U = -890.00 - (-2 × 2.4776) = -890.00 + 4.9552 = -885.04 ≈ -885.0 kJ/mol .

Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Thermodynamic Terms - System Surroundings and Types of Systems

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Gibbs Energy and Gibbs Energy Change and Equilibrium

For the combustion of 16 g of methane at 298 K ( Δ Hc = -890.30 kJ/mol , molar mass = 16 g/mol), what is Δ U ? ( R = 8.3

For CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l) , Δ ng = 1 - 3 = -2 . Then, RT = 8.314 × 298 × 10⁻³ = 2.4776 kJ . Using Δ H = Δ U + Δ ng RT , Δ U = -890.30 - (-2 × 2.4776) = -890.30 + 4.9552 = -885.34 kJ/mol .

Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Gibbs Energy and Gibbs Energy Change and Equilibrium

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First Law of Thermodynamics and Enthalpy and Internal Energy

Using bond enthalpies (C-H = 413 kJ/mol, O=O = 498 kJ/mol, C=O = 803 kJ/mol, O-H = 467 kJ/mol), calculate Δ H for CH₄(g)

Bonds broken: 4(C-H) + 2(O=O) = 4 × 413 + 2 × 498 = 1652 + 996 = 2648 kJ. Bonds formed: 2(C=O) + 4(O-H) = 2 × 803 + 4 × 467 = 1606 + 1868 = 3474 kJ. Δ H = 2648 - 3474 = -826 kJ/mol.

Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: First Law of Thermodynamics and Enthalpy and Internal Energy

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Laws of Chemical Combination - Conservation Mass Definite Multiple

What volume of O₂ at STP is required to burn 6 g of CH₄ completely to CO₂ and H₂O? (Molar mass: CH₄ = 16 g/mol)

Reaction: CH₄ + 2O₂ → CO₂ + 2H₂O. Moles of CH₄ = 6/16 = 0.375 mol. 1 mol CH₄ needs 2 mol O₂; 0.375 mol needs 0.75 mol. Volume = 0.75 × 22.4 = 16.8 L.

Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Laws of Chemical Combination - Conservation Mass Definite Multiple

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