The reaction

$2$CH$4($g$)$C$2$H$2($g$)+3$H$2($g$)$

has an equilibrium constant KP $=94\mathrm{.}5$ at $298$ K$.$

If $7\mathrm{.}00$ mol

of CH$4$

$,4\mathrm{.}75$ mol

of C$2$H$2$

$,$ and $10\mathrm{.}90$ mol

of H$2$

are added to a reaction vessel with a volume of $5\mathrm{.}20$ L

at $298$ K$,$ what net reaction will occur?