question_answer

What would be the reduction potential of an electrode at 298 K, which originally contained \[\text{1M}{{\text{K}}_{\text{2}}}\text{C}{{\text{r}}_{\text{2}}}{{\text{O}}_{\text{7}}}\] solution in acidic buffer solution of pH = 1.0 and which was treated with 50% of the Sn necessary to reduce all \[\text{C}{{\text{r}}_{\text{2}}}{{\text{O}}_{\text{7}}}^{2-}\] to \[\text{C}{{\text{r}}^{3+}}\]. Assume pH of solution remains constant. Given: \[\text{E}_{\text{C}{{\text{r}}_{\text{2}}}\text{O}\frac{\text{2-}}{\text{7}}\text{/C}{{\text{r}}^{\text{3+}}}\text{,}{{\text{H}}^{\text{+}}}}^{\text{0}}\]\[=1.33V,\log 2=0.3,\] \[\frac{2.303RT}{F}=0.06\]

A)  1.285 V               

B)  1.193 V

C)  1.187 V               

D)  None of these