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The equilibrium between, gaseous isomers A, B and C can be represented as
\( \mathrm{P} \)
Reaction Equilibrium constant
W.
\( \begin{array}{lll}\mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g}) & : & \mathrm{K}_{1}=? \\ \mathrm{~B}(\mathrm{~g}) \rightleftharpoons \mathrm{C}(\mathrm{g}) & : & \mathrm{K}_{2}=0.4 \\ \mathrm{C}(\mathrm{g}) \rightleftharpoons \mathrm{A}(\mathrm{g}) & : & \mathrm{K}_{3}=0.6\end{array} \)
If one mole of \( A \) is taken in a closed vessel of volume 1 litre, then
(A) \( [\mathrm{A}]+[\mathrm{B}]+[\mathrm{C}]=1 \mathrm{M} \) at any time of the reactions
(B) Concentration of \( \mathrm{C} \) is \( 4.1 \mathrm{M} \) at the attainment equilibrium in all the reactions
(C) The value of \( \mathrm{K}_{1} \) is \( \frac{1}{0.24} \)
(D) Isomer [A] is least stable as per thermodynamics.
(1) C, D
(2) A, C, D
(3) A, B, C
(4) A, C
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