The iron in a $6\mathrm{.}24g$ sample containing $F{e}_2{O}_3$ is reduced to$.F{e}^{2+}.$ The $F{e}^{2+}$ is titrated with $10\mathrm{.}48ml$ of $0\mathrm{.}124M{K}_{2}C{r}_2{O}_7$ in an acid solution $6F{e}^{2+}+C{r}_2{O}_7^{2+}+14H^{+}F{e}^{3+}+2C{r}^{3+}+\mathrm{.}7H_{2}O($l$)$

What is the $\%$ Fe in the sample?