Iron can be extracted from the iron(III) oxide found in ironores (such as haematite) via an oxidation-reductionreaction with carbon. The thermochemical equation for thisprocess is:2 Fe2O3(s) + 3 C(s) → 4 Fe(1) + 3 CO2(9)ΔΗ= +467.9 kJHow much heat (in kJ) is needed to convert 522 g Fe,O, into pure iron in the2.presence of excess carbon?kJWhen 1.38x107 kJ of heat is added to Fe,0, in the presence of excess carbon, howmany kilograms of Fe can be produced ?kg

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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(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

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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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