Given the standard half-cell potentials (Eo) of the following as
Zn=Zn2++2e−; Eo=+0.76V Fe=Fe2++2e−; Eo=+0.41V
Then the standard e.m.f. of the cell with the reaction Fe2++Zn→Zn2++Fe is?
−0.35V
+0.35V
+1.17V
−1.17V
A
−0.35V
B
−1.17V
C
+0.35V
D
+1.17V
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Solution
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Zn+2+2e−→Zn ; Eo=−0.76V (SRP) (Anode)
Fe+2+2e−→Fe ; Eo=−0.41V (SRP) (Cathode)
Eocell=E+Fe+2/Fe−EoZn+2/Zn
=−0.41+0.76=0.35V.
Hence, the correct option is B
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