A) 0.167
B) 0.6
C) 0.2
D) 0.4
Correct Answer: B
Solution :
| [b] The required equation is \[2KMn{{O}_{4}}+3{{H}_{2}}S{{O}_{4}}\xrightarrow{{}}\]\[{{K}_{2}}S{{O}_{4}}+2MnS{{O}_{4}}+3{{H}_{2}}O+~\underset{nascent\text{ }oxygen}{\mathop{5\left[ O \right]}}\,\] |
| \[2Fe\left( {{C}_{2}}{{O}_{4}} \right)+3{{H}_{2}}S{{O}_{4}}+3\left[ O \right]\xrightarrow{{}}\]\[F{{e}_{2}}{{\left( S{{O}_{4}} \right)}_{3}}+2C{{O}_{2}}+3{{H}_{2}}O\] |
| \[O\] required for 1 mol. of \[Fe({{C}_{2}}{{O}_{4}})\] is 1.5,5 \[O\] are obtained from 2 moles of \[KMn{{O}_{4}}\] |
| \[\therefore 1.5\text{ }\left[ O \right]\] will be obtained from \[=\frac{2}{5}\times 1.5=0.6\] moles of \[KMn{{O}_{4}}\]. |
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