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For the oxidation of iron to form iron(III) oxide: 4Fe(s) + 302(g) 2FE203(s) ASO = -549.73 JK1 at 298 K. The enthalpy of formation of Fe203(s) is -824.2 kJ mol What is the standard change in Gibbs free energy for this reaction at 298 K? Item equation/constant: AG° = AHO – TASO -660.4 k) O-988.0 kJ O-1484.6 kJ O -1812.2 k)

For the oxidation of iron to form iron(III) oxide: 4Fe(s) + 302(g) 2FE203(s) ASO = -549.73 JK1 at 298 K. The enthalpy of formation of Fe203(s) is -824.2 kJ mol What is the standard change in Gibbs free energy for this reaction at 298 K? Item equation/constant: AG° = AHO – TASO -660.4 k) O-988.0 kJ O-1484.6 kJ O -1812.2 k)

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
Problem 96QRT
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For the oxidation of iron to form iron(III) oxide: 4Fe(s) + 302(g)→ 2FE2O3(s) ASO = -549.73 JK1 at 298 K. The enthalpy of formation of Fe203(s) is –824.2 kJ mol. What is the standard change in Gibbs free energy for this reaction at 298 K? Item equation/constant: AG° = AHO – TASS O -660.4 kJ O -988.0 kJ O -1484.6 kJ O-1812.2 kJ
Transcribed Image Text:For the oxidation of iron to form iron(III) oxide: 4Fe(s) + 302(g)→ 2FE2O3(s) ASO = -549.73 JK1 at 298 K. The enthalpy of formation of Fe203(s) is –824.2 kJ mol. What is the standard change in Gibbs free energy for this reaction at 298 K? Item equation/constant: AG° = AHO – TASS O -660.4 kJ O -988.0 kJ O -1484.6 kJ O-1812.2 kJ
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