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10. Iron(III) oxide can be reduced by carbon monoxide. Fe₂O3(s) + 3CO(g) 2Fe(s) + 3CO₂(g)Use the following thermodynamic data at 298 K to determine the equilibrium constant K at this temperature. Substance: AH (kJ/mol): AGO (kJ/mol): S°(J/K mol): A) 7.0 x 10-6 B) 1.3 × 10-3 C) 2.2 × 104 D) 1.4 x 105 E) > 2.0 × 105 Fe₂O3(s) -824.2 -742.2 87.4 CO(g) -110.5 -137.2 197.7 Fe(s) 0 0 27.78 CO₂(g) -393.5 -394.4 213.7

10. Iron(III) oxide can be reduced by carbon monoxide. Fe₂O3(s) + 3CO(g) 2Fe(s) + 3CO₂(g)Use the following thermodynamic data at 298 K to determine the equilibrium constant K at this temperature. Substance: AH (kJ/mol): AGO (kJ/mol): S°(J/K mol): A) 7.0 x 10-6 B) 1.3 × 10-3 C) 2.2 × 104 D) 1.4 x 105 E) > 2.0 × 105 Fe₂O3(s) -824.2 -742.2 87.4 CO(g) -110.5 -137.2 197.7 Fe(s) 0 0 27.78 CO₂(g) -393.5 -394.4 213.7

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
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10. Iron(III) oxide can be reduced by carbon monoxide. Fe₂O3(s) + 3CO(g) ⇒ 2Fe(s) + 3CO₂(g)Use the following thermodynamic data at 298 K to determine the equilibrium constant K at this temperature. Substance: AHⓇ (kJ/mol): AG°f(kJ/mol): S°(J/K·mol): A) 7.0 x 10-6 B) 1.3 × 10-3 C) 2.2 x 104 D) 1.4 x 105 E) > 2.0 × 105 Fe₂O3(s) -824.2 -742.2 87.4 CO(g) -110.5 -137.2 197.7 Fe(s) 0 0 27.78 CO₂(g) -393.5 -394.4 213.7
Transcribed Image Text:10. Iron(III) oxide can be reduced by carbon monoxide. Fe₂O3(s) + 3CO(g) ⇒ 2Fe(s) + 3CO₂(g)Use the following thermodynamic data at 298 K to determine the equilibrium constant K at this temperature. Substance: AHⓇ (kJ/mol): AG°f(kJ/mol): S°(J/K·mol): A) 7.0 x 10-6 B) 1.3 × 10-3 C) 2.2 x 104 D) 1.4 x 105 E) > 2.0 × 105 Fe₂O3(s) -824.2 -742.2 87.4 CO(g) -110.5 -137.2 197.7 Fe(s) 0 0 27.78 CO₂(g) -393.5 -394.4 213.7
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