For the reaction 2H₂S(g) + 3O₂(g) → 2H₂O(l) + 2SO₂(g) , Δ ng = -3 . If Δ H = -1124.00 kJ/mol at 298 K, what is Δ U ? ( R
RT = 8.314 × 298 × 10⁻³ = 2.4776 kJ/mol . Using Δ H = Δ U + Δ ng RT , Δ U = -1124.00 - (-3 × 2.4776) = -1124.00 + 7.4328 = -1116.57 kJ/mol .
Ref: NCERT Class 11 Chemistry > Chapter 5: Thermodynamics > Topic: Gibbs Energy and Gibbs Energy Change and Equilibrium
