Calculate Change of Enthalpy- use Table A-14 1. Calcium carbonate breaks down into calcium oxide and carbon dioxide CaCO; (s) → CaO (s) + CO2 (g)
Calculate Change of Enthalpy- use Table A-14 1. Calcium carbonate breaks down into calcium oxide and carbon dioxide CaCO; (s) → CaO (s) + CO2 (g)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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number 1
![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)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F063622fb-d492-4548-9856-82f70650d79c%2F4ecace99-3ac2-47c7-90b6-6a8f11ca5e08%2F0oizmc_processed.png&w=3840&q=75)
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)
![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F063622fb-d492-4548-9856-82f70650d79c%2F4ecace99-3ac2-47c7-90b6-6a8f11ca5e08%2F7wld3zh_processed.png&w=3840&q=75)
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
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