JEE MAIN - Chemistry (2018 - 16th April Morning Slot - No. 12)
The gas phase reaction 2NO2(g) $$ \to $$ N2O4(g) is an exothermic reaction. The decomposition of N2O4, in equilibrium mixture of NO2(g) and N2O4(g), can be increased by :
lowering the temperature.
increasing the pressure.
addition of an inert gas at constant volume.
addition of an inert gas at constant pressure.
Explanation
2NO2 (g) $$\buildrel \, \over
\longrightarrow $$ N2O4 (g); $$\Delta $$H = $$-$$ ve
At equilibrium, N2O4 $$\rightleftharpoons$$ 2NO2 ; $$\Delta $$H = + ve
On adding the inert gas at constant pressure, the number of moles per unit volume of various reactants and products will decrease. Hence, the equilibrium will shift towards the direction in which there is increase in number of moles of gases. Therefore, in above case, reaction will move towards forward direction which will lead to the decomposition of dinitrogen tetraoxide (N2O4).
At equilibrium, N2O4 $$\rightleftharpoons$$ 2NO2 ; $$\Delta $$H = + ve
On adding the inert gas at constant pressure, the number of moles per unit volume of various reactants and products will decrease. Hence, the equilibrium will shift towards the direction in which there is increase in number of moles of gases. Therefore, in above case, reaction will move towards forward direction which will lead to the decomposition of dinitrogen tetraoxide (N2O4).
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