The gas phase reaction 2 NO 2( g ) arrow N 2 O 4( g ) is an exothermic reaction. The decomposition of N 2 O 4, in equilibrium mixture of NO 2( g ) and N 2 O 4( g ), can be increased by

Question

The gas phase reaction 2 NO 2( g ) arrow N 2 O 4( g ) is an exothermic reaction. The decomposition of N 2 O 4, in equilibrium mixture of NO 2( g ) and N 2 O 4( g ), can be increased by (A) lowering the temperature (B) increasing the pressure (C) addition of an inert gas at constant volume (D) addition of an inert gas at constant pressure

Tardigrade Admin · Accepted Answer

We have 2 NO 2( g ) leftharpoons N 2 O 4( g ) ; Δ H=- ve On adding the inert gas, 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 backward direction which will lead to the decomposition of dinitrogen tetraoxide ( N 2 O 4).

Q. The gas phase reaction 2NO2​(g)→N2​O4​(g) is an exothermic reaction. The decomposition of N2​O4​, in equilibrium mixture of NO2​(g) and N2​O4​(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

Q. The gas phase reaction $2 N O_{2} (g) \to N_{2} O_{4} (g)$ is an exothermic reaction. The decomposition of $N_{2} O_{4}$ , in equilibrium mixture of $N O_{2} (g)$ and $N_{2} O_{4} (g)$ , can be increased by