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For a gaseous reaction : $A_{(g)} ⇌ {3B}_{(g)} {+ C}_{(g)}, ΔH$ is positive and the reaction attains equilibrium at
1 bar total pressure and 400K. Identify the incorrect statements regarding the above reaction.

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$Δ G ° = 0$ for the above reaction at equilibrium

On increase of temperature, equilibrium will be shifted in forward direction

When inert gas is introduced into a rigid container containing above equilibria equilibrium

shifts towards left

If volume of vessel containing the above equilibria is increased without change in temperature

then partial pressure of B decreases as compared to original equilibrium partial pressure of B.

answer is B, C.

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Detailed Solution

$A_{(g)} ⇌ {3B}_{(g)} {+ C}_{(g)}; ΔH = + ve at 400 K$

$P_{total} at equilibrium = 1 bar$

$\Rightarrow$ On increasing T, reaction moves in forward direction.

$\Rightarrow$ On introducing inert gas at constant T. total pressure increases but partial pressure $\Rightarrow$ remains the same so no effect at equilibrium.

at 400 K, $K_{P} \neq 1 ({since P}_{total} = 1 bar)$

${ΔG}_{400K}^{0} = - {RT ln K}_{P} ¹ 0$

$\Rightarrow$ If V is increased, partial pressure of each species would be less than initital value.

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