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3. Iron (III) oxide + carbon monoxide produce iron + carbon dioxide (Fe = 0 KJ) Fe203 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g)

3. Iron (III) oxide + carbon monoxide produce iron + carbon dioxide (Fe = 0 KJ) Fe203 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g)

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.84QE
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Substance State AHs Substance State ΔΗ -45.9 -274.5 lead(IV) oxide lead(II) nitrate lead(II) sulfate ammonia ammonium chloride -314.4 -451.9 ammonium sulfate s -1180.9 -919.94 barium chloride -858.6 lithium chloride - 408.6 -483.1 -641.5 barium nitrate -768.2 lithium nitrate -1473.2 magnesium chloride magnesium oxide magnesium sulfate manganese(IV) oxide manganese(II) sulfate mercury(I) chloride mercury(II) chloride mercury(II) oxide (red) barium sulfate benzene +82.88 -601.6 benzene +49.080 1261.79 calcium carbonate s -1207.6 -520.0 calcium chloride -795.4 s -1065.3 calcium hydroxide -983.2 -264.2 calcium nitrate -938.2 -230.0 calcium oxide –634.9 -90.8 calcium sulfate carbon (diamond) carbon (graphite) -1434.5 methane -74.9 nitrogen dioxide nitrogen monoxide dinitrogen monoxide dinitrogen tetroxide +1.9 +33.2 0.00 +90.29 carbon diexide -393.5 +82.1 carbon monoxide -110.5 +9.2 copper(II) nitrate copper(II) oxide -302.9 oxygen (O2) ozone (O3) 0.00 -157.3 +142.7 copper(II) sulfate ethane tetraphosphorus decoxide potassium bromide potassium chloride potassium hydroxide potassium nitrate potassium sulfate silicon dioxide (quartz) -771.4 s -3009.9 - 393.8 -436.49 -83.8 ethyne (acetylene) hydrogen (H2) hydrogen bromide hydrogen chloride hydrogen fluoride hydrogen iodide hydrogen oxide (water) hydrogen oxide (water) hydrogen peroxide hydrogen peroxide hydrogen sulfide iodine (I2) +228.2 0.00 - 424.58 - 36.29 -494.6 -92.3 s -1437.8 -910.7 -273.3 +26.5 -241.8 silver chloride -127.01 ± 0.5 silver nitrate -120.5 1.-285.8 silver sulfide -32.59 8 -136.3 1 -187.8 sodium bromide -361.8 sodium chloride sodium hydroxide s - 385.9 -425.9 -20.6 0.00 sodium nitrate -467.9 iodine (I2) iron(I) chloride +62.4 sodium sulfate 1 -1387.1 8 -296.8 8 -395.7 -399.4 sulfur dioxide iron(II) oxide -272.0 sulfur trioxide -824.2 iron(III) oxide iron(II) sulfate tin(IV) chloride 1-511.3 -928.4 zinc nitrate -483.7 iron(II) sulfide lead(II) oxide AH is enthalpy of formation of the given substance from its elements. All values of AH are expressed as klimol at 25°C. Negative values of AH indicate exothermic reactions. s= solid, 1 = liquid, g = gas -100.0 zinc oxide -350.5 -217.3 zinc sulfate -980.14
Transcribed Image Text:Substance State AHs Substance State ΔΗ -45.9 -274.5 lead(IV) oxide lead(II) nitrate lead(II) sulfate ammonia ammonium chloride -314.4 -451.9 ammonium sulfate s -1180.9 -919.94 barium chloride -858.6 lithium chloride - 408.6 -483.1 -641.5 barium nitrate -768.2 lithium nitrate -1473.2 magnesium chloride magnesium oxide magnesium sulfate manganese(IV) oxide manganese(II) sulfate mercury(I) chloride mercury(II) chloride mercury(II) oxide (red) barium sulfate benzene +82.88 -601.6 benzene +49.080 1261.79 calcium carbonate s -1207.6 -520.0 calcium chloride -795.4 s -1065.3 calcium hydroxide -983.2 -264.2 calcium nitrate -938.2 -230.0 calcium oxide –634.9 -90.8 calcium sulfate carbon (diamond) carbon (graphite) -1434.5 methane -74.9 nitrogen dioxide nitrogen monoxide dinitrogen monoxide dinitrogen tetroxide +1.9 +33.2 0.00 +90.29 carbon diexide -393.5 +82.1 carbon monoxide -110.5 +9.2 copper(II) nitrate copper(II) oxide -302.9 oxygen (O2) ozone (O3) 0.00 -157.3 +142.7 copper(II) sulfate ethane tetraphosphorus decoxide potassium bromide potassium chloride potassium hydroxide potassium nitrate potassium sulfate silicon dioxide (quartz) -771.4 s -3009.9 - 393.8 -436.49 -83.8 ethyne (acetylene) hydrogen (H2) hydrogen bromide hydrogen chloride hydrogen fluoride hydrogen iodide hydrogen oxide (water) hydrogen oxide (water) hydrogen peroxide hydrogen peroxide hydrogen sulfide iodine (I2) +228.2 0.00 - 424.58 - 36.29 -494.6 -92.3 s -1437.8 -910.7 -273.3 +26.5 -241.8 silver chloride -127.01 ± 0.5 silver nitrate -120.5 1.-285.8 silver sulfide -32.59 8 -136.3 1 -187.8 sodium bromide -361.8 sodium chloride sodium hydroxide s - 385.9 -425.9 -20.6 0.00 sodium nitrate -467.9 iodine (I2) iron(I) chloride +62.4 sodium sulfate 1 -1387.1 8 -296.8 8 -395.7 -399.4 sulfur dioxide iron(II) oxide -272.0 sulfur trioxide -824.2 iron(III) oxide iron(II) sulfate tin(IV) chloride 1-511.3 -928.4 zinc nitrate -483.7 iron(II) sulfide lead(II) oxide AH is enthalpy of formation of the given substance from its elements. All values of AH are expressed as klimol at 25°C. Negative values of AH indicate exothermic reactions. s= solid, 1 = liquid, g = gas -100.0 zinc oxide -350.5 -217.3 zinc sulfate -980.14
Calculate Change of Enthalpy- use Table A-14 1. Calcium carbonate breaks down into calcium oxide and carbon dioxide CacO3 (s) → CaO (s) + CO2 (g) 2. Calcium hydroxide breaks down into calcium oxide and water (hydrogen oxide gas) Ca(OH)2 (s) → CaO (s) + H2O (g) 3. Iron (III) oxide + carbon monoxide produce iron + carbon dioxide (Fe = 0 KJ) Fe203 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g)
Transcribed Image Text:Calculate Change of Enthalpy- use Table A-14 1. Calcium carbonate breaks down into calcium oxide and carbon dioxide CacO3 (s) → CaO (s) + CO2 (g) 2. Calcium hydroxide breaks down into calcium oxide and water (hydrogen oxide gas) Ca(OH)2 (s) → CaO (s) + H2O (g) 3. Iron (III) oxide + carbon monoxide produce iron + carbon dioxide (Fe = 0 KJ) Fe203 (s) + 3 CO (g) → 2 Fe (s) + 3 CO2 (g)
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