Question

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 1

(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.

`\text{Moles of hematite}=\frac{\text{Mass of hematite}}{\text{Molar mass of hematite}}=(1000g)/(159.69g/mole)=6.26moles`

Now we have to calculate the moles of iron.

The given balanced reaction is,

`Fe_2O_3(s)+3CO(g)\rightarrow 2Fe(s)+3CO_2(g)`

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
`2* 6.26=12.52` moles of iron

Now we have to calculate the mass of iron.

`\text{Mass of iron}=\text{Moles of iron}* \text{Molar mass of iron}`

`\text{Mass of iron}=(12.52moles)* (55.8g/mole)=698.616g`

(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
`3* 6.26=18.78` moles of carbon dioxide

Now we have to calculate the mass of carbon dioxide.

`\text{Mass of }CO_2=\text{Moles of }CO_2* \text{Molar mass of }CO_2`

`\text{Mass of }CO_2=(18.78moles)* (44g/mole)=826.32g`

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