At 700 K, equilibrium constant for the reaction : $H_{2(g)} + I_{2(g)}$ ⇌ $2Hl_(g)$ is 54.8. If 0.5 $mol L^{–1}$ of $HI_(g)$ is present at equilibrium at 700 K, what are theconcentration of $H_{2(g)}$ and $I_{2(g)}$ assuming that we initially started with $HI_(g)$ and allowed it to reach equilibrium at 700 K?