When 10 mL of an aqueous solution of Fe^2+ ions was titrated in the presence of dil H_2 SO_4 using diphenylamine indicator, 15 mL of 0.02 M solution…

When $\displaystyle 10$ mL of an aqueous solution of $\displaystyle \mathrm{Fe}^{2+}$ ions was titrated in the presence of dil $\displaystyle \mathrm{H}_2 \mathrm{SO}_4$ using diphenylamine indicator, $\displaystyle 15$ mL of $\displaystyle 0.02$ M solution of $\displaystyle \mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ was required to get the end point. The molarity of the solution containing $\displaystyle \mathrm{Fe}^{2+}$ ions is $\displaystyle x \times 10^{-2} \mathrm{M}$. The value of $\displaystyle x$ is \_\_\_\_. (Nearest integer)