A sample (5.6 g) containing iron is completely dissolved in cold dilute $HCl$ to prepare a 250 mL of solution. Titration of 25.0 mL of this solution requires 12.5 mL of 0.03 M $KMnO_4$ solution to reach the end point. Number of moles of $Fe^{2+}$ present in 250 mL solution is x $\times$ 10 $-$ 2 (consider complete dissolution of $FeCl_2$). The amount of iron present in the sample is y% by weight. (Assume : $KMnO_4$ reacts only with $Fe^{2+}$ in the solution Use : Molar mass of iron as 56 g mol $-$ 1) The value of y is $\underline{\hspace{2cm}}$.