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Calculate the free energy change for the combustion of one mole of methane at 500°C: CH4 (g) +202 (8) CO2 (g) + 2H₂O(la) alculate the free energy change for the combustion of one mole of ethanol at 500°C: C₂H5OH(liq) + 302 (8) 2CO2(g) + 3H₂O(liq) 1 AG = 3CO2(g) + 4H2O(liq) AG= alculate the free energy change for the combustion of one mole of propane at 500°C: C3H8(e) + 502 (8) AG=

Calculate the free energy change for the combustion of one mole of methane at 500°C: CH4 (g) +202 (8) CO2 (g) + 2H₂O(la) alculate the free energy change for the combustion of one mole of ethanol at 500°C: C₂H5OH(liq) + 302 (8) 2CO2(g) + 3H₂O(liq) 1 AG = 3CO2(g) + 4H2O(liq) AG= alculate the free energy change for the combustion of one mole of propane at 500°C: C3H8(e) + 502 (8) AG=

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
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section16.9: Gibbs Free Energy And Biological Systems
Problem 16.13E
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Calculate the free energy change for the combustion of one mole of methane at 500°C: +202(g) → CO2 (g) + 2H₂O(l) CH4 (g) AG= Calculate the free energy change for the combustion of one mole of ethanol at 500°C: C₂H5OH (liq) + 302 (g) → 2CO2 (g) + 3H₂O(liq) AG = Calculate the free energy change for the combustion of one mole of propane at 500°C: C3H8 (8) +502 (6)→ 3CO2 (g) + 4H₂O(liq) AG=_ Calculate the free energy change for the combustion of one mole of butane at 500°C: C4H10 (liq) + 6% O2(g) → 4CO2 (g) + 5H₂O(liq) AG= the issue is keeping carbon dioxide to a minimum, which of the above fuels makes the most sense? That ich gives the most energy per carbon dioxide?
Transcribed Image Text:Calculate the free energy change for the combustion of one mole of methane at 500°C: +202(g) → CO2 (g) + 2H₂O(l) CH4 (g) AG= Calculate the free energy change for the combustion of one mole of ethanol at 500°C: C₂H5OH (liq) + 302 (g) → 2CO2 (g) + 3H₂O(liq) AG = Calculate the free energy change for the combustion of one mole of propane at 500°C: C3H8 (8) +502 (6)→ 3CO2 (g) + 4H₂O(liq) AG=_ Calculate the free energy change for the combustion of one mole of butane at 500°C: C4H10 (liq) + 6% O2(g) → 4CO2 (g) + 5H₂O(liq) AG= the issue is keeping carbon dioxide to a minimum, which of the above fuels makes the most sense? That ich gives the most energy per carbon dioxide?
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