question_answer

If the cell reaction are given as

(i) \[F{{e}^{2+}}(g)+2{{e}^{-}}\xrightarrow{{}}Fe(s)\,;\,{{E}^{o}}=-0.44\,V\]

(ii) \[2{{H}^{+}}(aq)+\frac{1}{2}{{O}_{2}}(g)+2{{e}^{-}}\to {{H}_{2}}O(\ell )\,;\,{{E}^{o}}=+1.23\,V\]the \[{{E}^{o}}\] for the reaction,

\[Fe(s)+2{{H}^{+}}+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}F{{e}^{2+}}(aq)+{{H}_{2}}O(\ell )\] is :

A) \[+1.67\,V\]   

B)                                    \[-1.67\,V\]

C) \[+0.79\,V\]         

D) \[-0.79\,V\]