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At 1200 the reduction of iron (III) oxide (Fe203) to elemental iron is nột spontan 2FE2O3(s) 4Fe(s) + 302(g) A;G° = +840 kJ the same temperature solid carbon spontaneously reacts with oxygen, to form C at by mixing carbon with Fe2O3 at this temperature the reduction can be made to p least 3 moles of carbon are present for every 2 moles of Fe2O3. (a) Write a balanced equation for the total reaction.

At 1200 the reduction of iron (III) oxide (Fe203) to elemental iron is nột spontan 2FE2O3(s) 4Fe(s) + 302(g) A;G° = +840 kJ the same temperature solid carbon spontaneously reacts with oxygen, to form C at by mixing carbon with Fe2O3 at this temperature the reduction can be made to p least 3 moles of carbon are present for every 2 moles of Fe2O3. (a) Write a balanced equation for the total reaction.

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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(ii) At 1200 °C, the reduction of iron (III) oxide (Fe2O3) to elemental iron is not spontaneous: 4Fe(s) + 302(g) 2FE2O3(s) A,G° = +840 kJ At the same temperature solid carbon spontaneously reacts with oxygen, to form CO2 gas. It is found that by mixing carbon with Fe2O3 at this temperature the reduction can be made to proceed, providing at least 3 moles of carbon are present for every 2 moles of Fe2O3. (a) Write a balanced equation for the total reaction. (b) Use the reaction stoichiometry to determine an upper limit for A,G, i.e. the least negative value possible, for the reaction of carbon with oxygen at this temperature.
Transcribed Image Text:(ii) At 1200 °C, the reduction of iron (III) oxide (Fe2O3) to elemental iron is not spontaneous: 4Fe(s) + 302(g) 2FE2O3(s) A,G° = +840 kJ At the same temperature solid carbon spontaneously reacts with oxygen, to form CO2 gas. It is found that by mixing carbon with Fe2O3 at this temperature the reduction can be made to proceed, providing at least 3 moles of carbon are present for every 2 moles of Fe2O3. (a) Write a balanced equation for the total reaction. (b) Use the reaction stoichiometry to determine an upper limit for A,G, i.e. the least negative value possible, for the reaction of carbon with oxygen at this temperature.
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