The equilibrium constant, $K_c,$ for the following

reaction is $1\mathrm{.}80{10}^{-4}$ at $298K.$

$N{H}_{4}HS(s)N{H}_3(g)+H_{2}S(g)$

Calculate the equilibrium concentration of $H_{2}S$

when $0\mathrm{.}432$ moles of $N{H}_{4}HS(s)$ are introduced

into a $1\mathrm{.}00L$ vessel at $298K.$

$[H_2(S)]=,M$