A) 0.6 moles
B) 0.4 moles
C) 7.5 moles
D) 0.2 moles
Correct Answer: A
Solution :
In ferrous oxalate ferrous and oxalate ions are oxidized. \[F{{e}^{2+}}\xrightarrow{{}}F{{e}^{3+}}+{{e}^{-}}\] \[{{C}_{2}}O_{4}^{2-}\xrightarrow{{}}2C{{O}_{2}}+2{{e}^{-}}\] \[MnO_{4}^{-}\xrightarrow{{}}M{{n}^{2+}},\] Thus eqn. will be \[3MnO_{4}^{-}+5Fe{{C}_{2}}{{O}_{4}}\xrightarrow{{}}\] \[\Rightarrow \]1 mole of ferrous oxalate requires 3/5 moles of \[KMn{{O}_{4}},\]i.e., 0.6 moles.
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