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Favorable conditions for formation of graphite are high pressure and 1ow temperature from equilibrium diamond $(d=3.5\mathrm{g}/\mathrm{ml})\rightleftharpoons$graphite $(d=2.3\mathrm{g}/\mathrm{ml});\mathrm{\Delta H}=-1.9\mathrm{kJ}/\mathrm{mole}$

For reaction ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO},\left(\mathrm{g}\right)$ degree of dissociation $\left(\mathrm{\alpha }\right)$ is $\sqrt{\frac{K_p}{4P+K_p}}$ where P is equilibrium pressure

For reaction ${\mathrm{Cl}}_2\left(g\right)+3{\widehat{F}}_2\left(g\right)\rightleftharpoons 2{\mathrm{ClF}}_3\left(g\right);\mathrm{\Delta H}=-329 \mathrm{kJ}$ dissociation of ${\mathrm{ClF}}_3\left(g\right)$ will be favorable by addition of inert gas at constant pressure

Reaction stops at equilibrium (microscopically)