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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 initiallyA. 80kgB. 124kgC. 44kgD. 100kg |
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Answer» `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 |
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