The reduction of iron(III) oxide (Fe2O3) to pure iron during the first step of steelmaking,2 Fe2O3(s) 4 Fe(s) + 302 (g)is driven by the high-temperature combustion of coke, a purified form of coal:C(s) + 0,(g) → CO₂ (g)Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG, of CO2 and Fe2O3 are-412. kJ/mol and -836. kJ/mol, respectively. Calculate the minimum mass of coke needed to produce 470. t of pure iron.(One metric ton, symbol t, equals 1000-kg.)Round your answer to 2 significant digits.kgx10

Step 1: First we need to get the net chemical reaction by balancing. We multiply the combustion of…

Answered: The reduction of iron(III) oxide…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 16.DCP

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The reduction of iron(III) oxide (Fe2O3) to pure iron during the first step of steelmaking, 2 FeO3(s) 4Fe(s) + 302(g) is driven by the high-temperature combustion of coke, a purified form of coal: C(s) + O2(g) → CO₂ (g) -> 11 ✓12 Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG, of CO2 and Fe2O3 are -447. kJ/mol and -818. kJ/mol, respectively. Calculate the minimum mass of coke needed to produce 7800. kg of pure iron. Round your answer to 2 significant digits. kg 5
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