Given are the following informations at 298 K.
$\begin{array}{llr} N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g) \\ Δ_{f} H^{\circ} / kJ {mol}^{- 1} 9.16 33.18 \\ Δ_{f} G^{\circ} / kJ {mol}^{- 1} 97.54 51.31 \end{array}$
The reaction is carried out in a closed vessel starting from $N_{2} O_{4}$ .
If the reaction is started with $N_{2} O_{4}$ at 1 atm pressure along with 0.5 atm of $N_{2}$ gas in the same vessel, the degree of dissociation of $N_{2} O_{4}$ at equilibrium relative to that of the reaction started only with $N_{2} O_{4}$ at 1 atm

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remains constant

increases

decreases

cannot be predicted

answer is A.

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Detailed Solution

The addition of inert gas at constant volume does not affect the degree of dissociation of $N_{2} O_{4}$ . The degree of dissociation may be calculated using the proportion of dissociating solute molecules. The formation of current-carrying free ions that split from the solute component at a specific temperature is another way to describe it.

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