What would be the reduction potential of an electrode at 298 K, which originally contained 1M ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ solution in acidic buffer soluton of pH = 1.0 and which was treated with 50% of the Sn necessary to reduce all ${\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}\text{ to }{\mathrm{Cr}}^{3+}$. Assume pH of solution remains constant. 

$\left[\text{ Given }:{\mathrm{E}}_{{\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}/{\mathrm{Cr}}^{3+},{\mathrm{H}}^{+}}^0=1.33 \mathrm{V},\log 2=0.3\right.$$\left.\frac{2.303\mathrm{RT}}{\mathrm{F}}=0.06\right]$