The equilibrium between gaseous isomers A, B and C can be represented as:
A(g) ⇌ B(g); K₁ = ?
B(g) ⇌ C(g); K₂ = 0.4
C(g) ⇌ A(g); K₃ = 0.6
If one mole of A is taken in a closed vessel of vo

Question

The equilibrium between gaseous isomers A, B and C can be represented as:
A(g) ⇌ B(g); K₁ = ?
B(g) ⇌ C(g); K₂ = 0.4
C(g) ⇌ A(g); K₃ = 0.6
If one mole of A is taken in a closed vessel of volume 1L, then

Prashant Kotian · Accepted Answer

Correct answer: A,C,D. The sum of the reactions gives a net change of zero, so K₁ × K₂ × K₃ = 1. K₁ × 0.4 × 0.6 = 1 => K₁ = 1 / 0.24 (Option C). At equilibrium, [B]/[A] = K₁ ≈ 4.17, [C]/[B] = 0.4. Thus, [B] > [C] > [A]. Thermodynamic stability is proportional to equilibrium concentration, making A the least stable isomer (Option D). Since it's a closed 1 L vessel and all are isomers, total moles remain 1, so [A] + [B] + [C] = 1 M (Option A). Therefore, correct answer is A,C,D.

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