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# Answer to Question #206163 in General Chemistry for Ali

Question #206163

Metal oxides are reduced in reactions that produce pure metal. If the percent yield of iron is 78% when hematite (Fe2O3) is reduced in a blast furnace and 72% when magnetite (Fe3O4) is reduced which ore would produce the greatest amount of iron per metric ton (1000kg) of reactant used?

1
2021-06-14T13:37:24-0400

The balanced equation 2Fe2O3 ---> 4Fe + 3O2 for hematite.

Mol. Mass Fe2O3 = 159.7 x 2 =319.4 kg

Atomic mass Fe = 55.845 x 4 = 223.4 kg

If all 1000 kg Fe2O3 reacted, the mass of Fe produced would be 223.4 kg Fe/319.4 kg Fe2O3 x 1000 kg Fe2O3 = 699.4 kg Fe. As the yield is 72%, the actual mass of Fe produced is 699.4 kg x 0.72 = 503.6 kg.

The balanced equation Fe3O4 ------> 3Fe + 2O2 for magnetite

Mol. Mass Fe3O4 = 55.845 x 3 = 231.5 kg

Atomic mass Fe = 55.845 x 3 = 167.5 kg

If all 1000 kg Fe3O4 reacted, the mass of Fe produced would be 167.5 kg/231.5 kg x 1000 kg = 723.5 kg.

As the yield was 78%, the actual mass of Fe is 564.4 kg. Magnetite produces the greater mass of Fe

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