Iron metal is obtained from the reaction of hematite [iron (iii) oxide, fe2o3] with carbon monoxide in a blast furnace. fe2o3 (s) + 3 co (g) > 2 fe (s) + 3 co2 (g) (a) calculate the number of grams of iron metal that can be obtained from 1.00 kg of hematite (assuming that you have enough co available for any reaction). feb) calculate the amount of co2 in grams that you you will get in this reaction, using the amount of hematite in (a). g co2

Answer :

(a) The number of grams of iron metal obtained, 698.616 g

(b) The number of grams of carbon dioxide used in the reaction, 826.32 g

Solution : Given,

Mass of hematite = 1 Kg = 1000 g

Molar mass of hematite = 159.69 g/mole

Molar mass of iron = 55.8 g/mole

Molar mass of carbon dioxide = 44 g/mole

(a) First we have to calculate the moles of hematite.

Now we have to calculate the moles of iron.

The given balanced reaction is,

From the balanced reaction, we conclude that

As, 1 mole of hematite react to give 2 moles of iron

So, 6.26 moles of hematite react to give moles of iron

Now we have to calculate the mass of iron.

(b) Now we have to calculate the moles of carbon dioxide.

From the balanced reaction we conclude that

As, 1 mole of hematite react to give 3 moles of carbon dioxide

So, 6.26 moles of hematite react to give moles of carbon dioxide

Now we have to calculate the mass of carbon dioxide.

Therefore, (a) The number of grams of iron metal obtained, 698.616 g

(b) The number of grams of carbon dioxide used in the reaction, 826.32 g