For the given reaction,
2 A(g) + B(g) → 2D(g)
∆ng = 2 – (3)
= –1 mole
Substituting the value of ∆Uθ in the expression of ∆H:
∆Hθ = ∆Uθ + ∆ngRT
= (–10.5 kJ) – (–1) (8.314 × 10–3 kJ K–1 mol–1 ) (298 K)
= –10.5 kJ – 2.48 kJ ∆Hθ = –12.98 kJ
Substituting the values of ∆Hθ and ∆Sθ in the expression of
∆Gθ : ∆Gθ = ∆Hθ – T∆Sθ
= –12.98 kJ – (298 K) (–44.1 J K–1 )
= –12.98 kJ + 13.14 kJ
∆Gθ = + 0.16 kJ
Since ∆Gθ for the reaction is positive, the reaction will not occur spontaneously.