A mixture of 0.4 mole of $H_2\left(g\right)$ and 0.2 mole of $B{r}_2\left(g\right)$ is heated  in a container of volume 1 litre at 700 K to achieve an equilibrium. The equilibrium constant  $\left[K_c\right]$ is  $2.5\times {10}^9$. Find out the value of $\frac{\left[B{r}_2\right]}{\left[HBr\right]}\times {10}^{10}.$ Here $\left[B{r}_2\right]$ and $\left[HBr\right]$ are the concentrations of $B{r}_2\left(g\right)$ and $HBr\left(g\right)$ respectively at equilibrium.