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: 2Fe2O3(�)+3C(�)→4Fe(�)+3CO2(�)Δ�o=+467.9kJ - How much heat (in kJ) is needed to convert 358 g Fe2O3 into pure iron in the presence of excess carbon? kJ - When 7.50 ×107 kJ of heat is added to Fe2O3 in the presence of excess carbon, how many kilograms of Fe can be produced ? kg
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: 2Fe2O3(�)+3C(�)→4Fe(�)+3CO2(�)Δ�o=+467.9kJ - How much heat (in kJ) is needed to convert 358 g Fe2O3 into pure iron in the presence of excess carbon? kJ - When 7.50 ×107 kJ of heat is added to Fe2O3 in the presence of excess carbon, how many kilograms of Fe can be produced ? kg
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.36QE: When lightning strikes, the energy can force atmospheric nitrogen and oxygen to react to make NO:...
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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:
2Fe2O3(�)+3C(�)→4Fe(�)+3CO2(�)Δ�o=+467.9kJ
- How much heat (in kJ) is needed to convert 358 g Fe2O3 into pure iron in the presence of excess carbon? kJ
- When 7.50 ×107 kJ of heat is added to Fe2O3 in the presence of excess carbon, how many kilograms of Fe can be produced ? kg
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