According to Le chatelier's principle-
$(a)$ addition of an inert gas at constant pressure will increase volume and equilibirium shifts towards more number of molecules.
$(b)$ Decomposition of $N_2O_4$ will be endothermic, so reaction wil move in forward reaction when temperature is increased.So, It is incorrect. It will not effect reaction (volume is constant)
$(c)$ Increasing the pressure on a gas reaction shifts the position of equilibirium towards
the side with fewer molecules. So, It will move in backward direction which leads to formation of $N_2O_4$ from $NO_2$
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
$C{H_3} - \mathop {\mathop {\mathop {\mathop C\limits^| }\limits^{Cl} - }\limits_{|\,\,\,\,} }\limits_{OH} C{H_2}CH = CHC{H_3}$