# Q6.19. For the reaction2 A(g) + B(g) → 2D(g)ΔU 0 = ?10.5 kJ and ΔS0 = ?44.1 J\k.Calculate ΔG0 for the reaction, and predict whether the reactionmay occur spontaneously

Aman Bansal
592 Points
11 years ago

Dear Student,

For the given reaction,
2 A(g) + B(g) → 2D(g)
Δng = 2 – (3)
= –1 mole
Substituting the value of ΔUθ in the expression of ΔH:
ΔHθ = ΔUθ + ΔngRT
= (–10.5 kJ) – (–1) (8.314 × 10–3 kJ K–1 mol–1) (298 K)
= –10.5 kJ – 2.48 kJ
ΔHθ = –12.98 kJ
Substituting the values of ΔHθ and ΔSθ in the expression of ΔGθ:
ΔGθ = ΔHθTΔSθ
= –12.98 kJ – (298 K) (–44.1 J K–1)
= –12.98 kJ + 13.14 kJ
ΔGθ = + 0.16 kJ
Since ΔGθ for the reaction is positive, the reaction will not occur spontaneously.

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Aman Bansal