A battery is constructed of Cr and \[N{{a}_{2}}C{{r}_{2}}{{O}_{7}}\]. The unbalanced chemical equation when such a battery discharges is following \[N{{a}_{2}}C{{r}_{2}}{{O}_{7}}+Cr+{{H}^{+}}\to C{{r}^{3+}}+{{H}_{2}}O+N{{a}^{+}}\] If one Faraday of electricity is passed through the battery during the charging, the number of moles of \[C{{r}^{\text{3+}}}\] removed from the solution is

• A. \[\frac{4}{3}\]                          
• B. \[\frac{1}{3}\]
• C. \[\frac{3}{3}\]                          
• D. \[\frac{2}{3}\]