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Moles = 40 / 56 = 0.7143 mol, Δ T = 100 - 20 = 80 K, qp = nCpΔ T = 0.7143 × 25.1 × 80 = 1434.3 J = 1.434 kJ.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Third Law of Thermodynamics and Applications
Moles = 27 / 27 = 1 mol, Δ T = 20 K, q = nCpΔ T = 1 × 24 × 20 = 480 J = 0.48 kJ.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Heat Capacity and Calorimetry and Measurement of Enthalpy
Moles of CO₂ = 22 / 44 = 0.5 mol . For C(s) + O₂(g) → CO₂(g) , Δ H = -393.5 kJ/mol . Heat released = 0.5 × 393.5 = 196.75 kJ (positive, as heat is released in exothermic reaction).
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Heat Capacity and Calorimetry and Measurement of Enthalpy
Moles = 54 / 18 = 3 mol, Δ T = 80 - 20 = 60 K, qp = nCpΔ T = 3 × 75.3 × 60 = 13554 J = 13.55 kJ.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Gibbs Energy and Gibbs Energy Change and Equilibrium
Moles = 32 / 32 = 1 mol, Δ T = 130 - 30 = 100 K, qp = nCpΔ T = 1 × 22.7 × 100 = 2270 J = 2.27 kJ.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Gibbs Energy and Gibbs Energy Change and Equilibrium
q = m × C × Δ T = 40 × 4.18 × 10 = 1672 J = 1.672 kJ.
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: First Law of Thermodynamics and Enthalpy and Internal Energy
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