To develop general equation of standard Gibbs energy of reaction Δ G 0 N 2 + 3H 2 → 2 NH 3 Concept Introduction : Gibbs change of Energy is given as below, Δ G o = Δ H 0 0 − T T O ( Δ H 0 0 − Δ G 0 0 ) + R ∫ T 0 T Δ C P R d T − R T ∫ T 0 T Δ C P R T d T The integral of rate of change of molar heat capacity is the enthalpy change as given below: - Where, ∫ T 0 T C P R d T = A . T 0 ( τ − 1 ) + B 2 T 0 2 ( τ 2 − 1 ) + C 3 T 0 3 ( τ 3 − 1 ) + D T 0 ( τ − 1 τ ) ∫ T 0 T C P R d T T = A ln τ + [ B T 0 + ( C T 0 2 + D T 0 2 ) ( τ + 1 τ ) ] ( τ − 1 ) A, B, C, D are constants T o = Initial temperature = 25 0 C = 298 K T = Final temperature τ = T T o = T 298 C p = Molar heat capacity R = Universal Gas constant = 8.314 J/molK Δ H o = ∑ i v i H i o = Heat of formation of products − Heat of formation of reactants Δ H 298 0 = Heat of formation at 298 K Δ H 0 0 = Standard Heat of Reaction Δ G 298 0 = Standard Gibbs Energy of reaction at 298 K Δ G 0 = Standard Gibbs Energy of reaction
To develop general equation of standard Gibbs energy of reaction Δ G 0 N 2 + 3H 2 → 2 NH 3 Concept Introduction : Gibbs change of Energy is given as below, Δ G o = Δ H 0 0 − T T O ( Δ H 0 0 − Δ G 0 0 ) + R ∫ T 0 T Δ C P R d T − R T ∫ T 0 T Δ C P R T d T The integral of rate of change of molar heat capacity is the enthalpy change as given below: - Where, ∫ T 0 T C P R d T = A . T 0 ( τ − 1 ) + B 2 T 0 2 ( τ 2 − 1 ) + C 3 T 0 3 ( τ 3 − 1 ) + D T 0 ( τ − 1 τ ) ∫ T 0 T C P R d T T = A ln τ + [ B T 0 + ( C T 0 2 + D T 0 2 ) ( τ + 1 τ ) ] ( τ − 1 ) A, B, C, D are constants T o = Initial temperature = 25 0 C = 298 K T = Final temperature τ = T T o = T 298 C p = Molar heat capacity R = Universal Gas constant = 8.314 J/molK Δ H o = ∑ i v i H i o = Heat of formation of products − Heat of formation of reactants Δ H 298 0 = Heat of formation at 298 K Δ H 0 0 = Standard Heat of Reaction Δ G 298 0 = Standard Gibbs Energy of reaction at 298 K Δ G 0 = Standard Gibbs Energy of reaction