Chemical EquilibriumHard
Question
In the following equilibrium N2O4(g) $\rightleftharpoons$2NO2(g), when 5 moles of each is taken and the temperature is kept at 298 K, the total pressure was found to be 20 bar. Given ΔfGo [N2O4(g)] = 100 kJ/mol; ΔfGo [NO2(g)] = 50 kJ/mol.
Options
A.KP for the reaction is 1.0 bar.
B.ΔGo for the reaction is zero at 298 K.
C.Under the given condition, the reaction is mainly occurring in backward direction.
D.The mixture taken is at equilibrium.
Solution
$\Delta G^{o} = 2 \times \Delta_{f}G_{NO_{2}(g)}^{o} - \Delta_{f}G_{N_{2}O_{4}(g)}^{o} = 0 \Rightarrow K_{P}^{o} = 1$
Now, $\Delta G = \Delta G^{o} + RT.\ln Q = 0 + RT.\ln\frac{P_{NO_{2}}^{2}}{P_{N_{2}O_{4}}} = RT.\ln\frac{10^{2}}{10} = \text{Positive}$
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