Consider the following reaction


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 $(a, b)$, the direction in which the equilibrium shifts is:

(a) Temperature is decreased

(b) Pressure is increased by adding $\mathrm{N}_{2}$ at constant $\mathrm{T}$


  1. (a) towards reactant, (b) no change

  2. (a) towards product, (b) towards reactant

  3. (a) towards product, (b) no change

  4. (a) towards reactant, (b) towards product

Correct Option: 1


$\Delta \mathrm{H}^{\circ}>0 \quad \mathrm{~T} \downarrow$ equation shifts back ward.

$\mathrm{N}_{2}$ is treated as inert gas in this case hence no effect on equilibrium.


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