The standard electrode potential for the half cell reactions are : {\Zn}^{++}+2 {\e}^{-} \to {\Zn} {\E}^{\circ}=-0.76 {\V} {\Fe}^{++}+2 {\e}^{-} \to {\Fe} {\E}^{\circ}=-0.44 {\V} The E.M.F. of the cell reaction : {\Fe}^{++}+ {\Zn} \to {\Zn}^{++}+ {\Fe} is

KCET 2009 Chemistry Solved Paper

Question : 38 of 60

Marks: +1, -0

The standard electrode potential for the half cell reactions are :
‌Zn+++2e−→Zn‌E∘=−0.76V
‌Fe+++2e−→Fe‌E∘=−0.44V
The E.M.F. of the cell reaction : Fe+++Zn→Zn+++Fe is

+1.20V
+0.32V
−0.32V
−1.20V

Validate

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