A) 10
B) 5
C) 6
D) 2
Correct Answer: B
Solution :
The balanced equation of acidified\[FeS{{O}_{4}}\]with \[KMn{{O}_{4}}\]is \[2KMn{{O}_{4}}+8{{H}_{2}}S{{O}_{4}}\underset{ferrous\text{ }sulphate}{\mathop{+10FeS{{O}_{4}}}}\,\xrightarrow{{}}\] \[{{K}_{2}}S{{O}_{4}}+2MnS{{O}_{4}}\underset{ferric\text{ }sulphate}{\mathop{+5F{{e}_{2}}{{(S{{O}_{4}})}_{3}}+}}\,8{{H}_{2}}O\] \[\because \] 2 mole of KMn04 oxidised = 10 moles of \[FeS{{O}_{4}}\] \[\therefore \]1 mole of KMn04 will oxidise\[=\frac{10}{2}=5\]moles of\[FeS{{O}_{4}}\]
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