The equilibrium constant, $K,$ for the following reaction is $1\mathrm{.}80{10}^{-2}$ at $698K.$

$2HI(g)[2]H_2(g)+I_2(g)$

An equilibrium mixture of the three gases in a $1\mathrm{.}00L$ flask at $698K$ contains $0\mathrm{.}324$MHI,$4\mathrm{.}35{10}^{-2}M{H}_2$ and $4\mathrm{.}35{10}^{-2}M{I}_2.$ What will be the concentrations of the three gases once equilibrium has been reestablished, if $0\mathrm{.}193$mol of $HI(g)$ is added to the flask?

$[HI]=,M$

$[H_2]=,M$

$[I_2]=,M$