Consider the following reaction for which the change in enthalpy is positive.

$2 \mathrm{A}( \mathrm{g})+\mathrm{B}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{C}\left(\mathrm{g}\right)+\mathrm{D}\left(\mathrm{g}\right)$

Which of the following will not affect the equilibrium?

$\begin{array}{l}2\mathrm{A}\left(\mathrm{g}\right)+\mathrm{B}\left(\mathrm{g}\right) \rightleftarrows \mathrm{C}\left(\mathrm{g}\right) +\mathrm{D}\left(\mathrm{g}\right);∆\mathrm{H}=+\mathrm{ve}\\ \mathrm{\Delta n}=2-3\\ =–1\end{array}$

$\therefore$    Increase in pressure favours forward reaction
$\because$    the reaction is endothermic, forward reaction is favoured at high temperature.
Addition of A (or) B and removal of C (or) D favours forward reaction
Catalyst has no influence on equilibrium state. It increases both rate of forward reaction and rate of backward reaction to the same extent.