Chemistry - Redox Reactions Question with Solution | TestHub

A sample $(5.6\mathrm{g})$ containing iron is completely dissolved in cold dilute $\mathrm{HCl}$ to prepare a $250\mathrm{mL}$ of solution. Titration of $25.0\mathrm{mL}$ of this solution requires $12.5\mathrm{mL}$ of $0.03\mathrm{M}{\mathrm{KMnO}}_4$ solution to reach the end point. Number of moles of ${\mathrm{Fe}}^{2+}$ present in $250\mathrm{mL}$ solution is $\mathbf{x}\times 10^{-2}$ (consider complete dissolution of ${\mathrm{FeCl}}_2$ ). The amount of iron present in the sample is $\mathbf{y}\%$ by weight.
(Assume: ${\mathrm{KMnO}}_4$ reacts only with ${\mathrm{Fe}}^{2+}$ in the solution Use: Molar mass of iron as $56\mathrm{g}{\mathrm{mol}}^{-1}$ )
The value of$\mathrm{y}$is________ .