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1. An iron ore (500 tonnes) contained 12% iron oxide (Fe2O3) by mass. The iron oxide was reduced
in the blast furnace to form iron: Fe2O3 (s) + 3CO(g) → 2Fe(l) + 3CO2(g). (1 tonne = 1 x 106g)

(i) Calculate the mass of iron oxide (Fe2O3) found in the 500 tonnes of iron ore.
mass of iron oxide = ............................... tonnes [2]

(ii) How many moles of iron oxide (Fe2O3) were present?
moles of iron oxide = ............................... moles [2]

(iii) What mass of iron can be formed from this quantity of ore?
mass of iron = ............................... tonnes [2]

I have done parts 1 and 2 but i am stuck on part 3, any help is appreciated x
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4. (Original post by unidentified__)
An iron ore (500 tonnes) contained 12% iron oxide (Fe2O3) by mass. The iron oxide was reduced
in the blast furnace to form iron: Fe2O3 (s) + 3CO(g) → 2Fe(l) + 3CO2(g). (1 tonne = 1 x 106g)

(i) Calculate the mass of iron oxide (Fe2O3) found in the 500 tonnes of iron ore.
mass of iron oxide = ............................... tonnes [2]

(ii) How many moles of iron oxide (Fe2O3) were present?
moles of iron oxide = ............................... moles [2]

(iii) What mass of iron can be formed from this quantity of ore?
mass of iron = ............................... tonnes [2]

I have done parts 1 and 2 but i am stuck on part 3, any help is appreciated x
I think you're overthinking things; it's really not as hard as it looks (she says )

So, you use your answer for the number of moles of Fe2CO3 and multiply that by two, because the ratio of Fe2CO3 to Fe is 1:2, as shown in the equation. You then multiply that by the relative atomic mass of Fe, which is 55.8, and there you have your mass of iron if you go ahead and convert use masses in grams or kilograms, divide by 1,000,000 and 1000 respectively. You should get something around about 39 tonnes hope that helped

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