For the gaseous phase reaction $2 A + B ⇌ 2 C + D,$ initially there are 2 mole each of A & B. If 0.4 mol of D is present at equilibrium at a given T & P, incorrect relationship is

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$P_{A} < P_{B} & P_{D} < P_{C}$

$P_{C} = 2 P_{D} & P_{A} = 3 P_{B} / 4$

$P_{A} > P_{D} & P_{B} > P_{C}$

$P_{A} = P_{C} & P_{B} = P_{C}$

answer is B.

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Detailed Solution

Consider the following equilibrium.

$2 A + B ⇌ 2 C + D$

Initial moles 2 2 0 0

Reacted moles -0.8 -0.4 0.8 0.4

Reacted moles

At equilibrium 1.2 1.6 0.8 0.4 .

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