A) \[\frac{2}{5}\]
B) \[\frac{3}{5}\]
C) \[\frac{4}{5}\]
D) 1
Correct Answer: B
Solution :
\[F{{e}^{2+}}\to F{{e}^{3+}}+{{e}^{-}}\] \[\begin{align} & CO{{O}^{-}} \\ & | \\ & CO{{O}^{-}}\to 2C{{O}_{2}}+2{{e}^{-}} \\ \end{align}\] Ferrous oxalate on oxidation loses 3 electrons. Permanganate ion on reduction gains 5 electrons. Thus, 1 mole of ferrous oxalate will need 3/5 moles of \[KMn{{O}_{4}}\] for complete oxidation.You need to login to perform this action.
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