Consider the following reaction :
$\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g}) ; \Delta \mathrm{H}^{0}=+58 \mathrm{~kJ}$
For each of the following cases ((i), (ii)), the direction in which the equilibrium shifts is :
(i) Temperature is decreases
(ii) Pressure is increased by adding $\mathrm{N}_{2}$ at constant $\mathrm{T}$.
Correct Option: , 3
(i) As reaction is endothermic $(\Delta \mathrm{Hz}=+\mathrm{ve})$ so on decrease in temperature equilibrium will shift towards reactant side.
(ii) On increase in pressure by adding inert gas $\left(\mathrm{N}_{2}\right)$ at same temperature, no shifting will take place. The equilibrium changes only if the added gas is a reactant or product involved in the reaction.
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