Iron is prepared from one of its ore hematite `Fe_(2)O_(3)` by reaction with carbon as follows:
`Fe_(2)O_(3)(s)+C(s)rarrFe(s)+CO_(2)(g)uparrow`
Above reaction occur in an open furnance.
If carbon was taken in limiting quality, as a result finally 100kg of crude iron (a mixture of `Fe_(2)O_(3)` and Fe) was obtained. And crude iron has `56%` pure Fe. Then what mass of `Fe_(2)O` was taken initially

Options

A. 80kg
B. 124kg
C. 44kg
D. 100kg

Explanation

`2Fe_(2)O_(3)(s)+3C(s)rarr4Fe(s)+3CO_(2)`
after reaction 44kg 56 kg
`n_(Fe(2)O_(3))"used"=n_(Fe)=("formed")/(2)=(56)/(56)xx(10^(3))/(2)`
`w_(Fe_(2)O_(3))"used"=(160)/(2)kg=80kg`
`w_(Fe_(2)O_(3))` initially taken =80+44=124kg