Iron can be extracted from the iron(III) oxide found in iron ores (such as haematite) via an oxidation-reduction reaction with carbon. The thermochemical equation for this process is: 2 Fe2O3(s) + 3 C(s) → 4 Fe(1) + 3 CO2(g) AH° = +467.9 kJ How much heat (in kJ) is needed to convert 522 g Fe,O, into pure iron in the presence of excess carbon? kJ

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Iron can be extracted from the iron(III) oxide found in iron
ores (such as haematite) via an oxidation-reduction
reaction with carbon. The thermochemical equation for this
process is:
2 Fe2O3(s) + 3 C(s) → 4 Fe(1) + 3 CO2(9)
ΔΗ
= +467.9 kJ
How much heat (in kJ) is needed to convert 522 g Fe,O, into pure iron in the
2.
presence of excess carbon?
kJ
When 1.38x107 kJ of heat is added to Fe,0, in the presence of excess carbon, how
many kilograms of Fe can be produced ?
kg
Transcribed Image Text:Iron can be extracted from the iron(III) oxide found in iron ores (such as haematite) via an oxidation-reduction reaction with carbon. The thermochemical equation for this process is: 2 Fe2O3(s) + 3 C(s) → 4 Fe(1) + 3 CO2(9) ΔΗ = +467.9 kJ How much heat (in kJ) is needed to convert 522 g Fe,O, into pure iron in the 2. presence of excess carbon? kJ When 1.38x107 kJ of heat is added to Fe,0, in the presence of excess carbon, how many kilograms of Fe can be produced ? kg
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