Using values from Appendix C, calculate the standard enthalpy change for each of the following reactions: (a) 2 SO2(g) + O2(8) 2 SO3(8) > MgO(s) + H2O(1) N2(8) + 4 H2O(g) (b) Mg(OH)2(s) (c) N2O4(8) + 4 H2(8) (d) SiCl,(1) + 2 H;O(1) SIO2(s) + 4 HC1(8) -
Using values from Appendix C, calculate the standard enthalpy change for each of the following reactions: (a) 2 SO2(g) + O2(8) 2 SO3(8) > MgO(s) + H2O(1) N2(8) + 4 H2O(g) (b) Mg(OH)2(s) (c) N2O4(8) + 4 H2(8) (d) SiCl,(1) + 2 H;O(1) SIO2(s) + 4 HC1(8) -
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.116QP: Ethylene glycol, HOCH2CH2OH, is used as antifreeze. It is produced from ethylene oxide, C2H4O, by...
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Transcribed Image Text:APPENDIX
Thermodynamic Quantities
for Selected Substances
at 298.15 K (25 °C)
AH
(ki/mol)
AG?
(k/mol)
AH
(kj/mol)
AG
(kj/mol)
S°
Substance
(1/mol-K)
Substance
(1/mol-K)
Aluminum
CHulg)
-124.73
- 15.71
310.0
Al(s)
28.32
-1476
-15.0
231.0
AICH (1)
-705.6
-630.0
109.3
CH, (g)
82.9
129.7
269.2
- 1669.8
- 1576.5
51.00
CH, (1)
CHOH(g)
49.0
124.5
172.8
Barium
-201.2
- 161.9
237.6
CH,OH(I)
CH,OH(g)
C,H,OH(I)
CH06(s)
Co(g)
CO(g)
CH,COOH(I)
-238.6
- 166.23
126.8
Ba(s)
63.2
-235.1
- 168.5
282.7
BaCO,(s)
BaO(9)
- 1216.3
-1137.6
112.1
-553.5
-525.1
70.42
-277.7
- 174.76
160.7
-1273.02
-910.4
212.1
Beryllium
-110.5
-137.2
197.9
Be(s)
9.44
-393.5
-394.4
213.6
BeO(s)
-608.4
-579.1
13.77
-4870
-392.4
159.8
Be(OH),(4)
-905.8
-817.9
50.21
Cesium
Bromine
Cslg)
76.50
49.53
175.6
Brg)
Br" (aq)
Bry (g)
Bry (1)
HBr(g)
Calcium
111.8
82.38
174.9
- 120.9
- 102.8
80.71
Cs(f)
2.09
0.03
92.07
30.71
3.14
245.3
Cs(s)
85.15
152.3
CSCI()
-442.8
-414.4
101.2
-36.23
-53.22
198.49
Chlorine
121.7
105.7
165.2
179.3
cr(ag)
-167.2
-131.2
56.5
Calg)
Ca(s)
145.5
154.8
222.96
41.4
CaCO,(s, calcite) -1207.1
HCI(ag)
-167.2
-131.2
56.5
-1128.76
92.88
HCI(g)
-92.30
-95.27
186.69
CaCl,(s)
CaF,(s)
-795.8
-748.1
104.6
- 1219.6
-1167.3
68.87
Chromium
CaO()
-635.5
-604.17
39.75
Cre)
397.5
352.6
174.2
Ca(OH),(s)
CasO(s)
-986.2
- 898.5
83.4
Cr(s)
23.6
- 1434.0
- 1321.8
106.7
-1139.7
-1058.1
81.2
Carbon
Cobalt
718.4
672.9
158.0
Colg
439
393
179
C(s, diamond)
1.88
284
Co(s)
2.43
28.4
C(s. graphite)
5.69
Copper
Culg)
- 106.7
-64.0
309.4
338.4
298.6
166.3
CCL(1)
CF,(g)
CH (g)
C,H(g)
C,H(g)
- 139.3
-68.6
214.4
Cu(s)
33.30
-679.9
-635.1
262.3
CuCl,()
CuO)
-205.9
- 161.7
108.1
-74.8
-50.8
186.3
-156.1
- 128.3
42.59
226.77
209.2
200.8
Cu,O(s)
-170.7
-147.9
92.36
52.30
68.11
219.4
Fluorine
-84.68
-32.89
229.5
158.7
F(g)
F"(aq)
80.0
61.9
C,H(g)
- 103.85
-23.47
269.9
-332.6
-278.8
- 13.8
Transcribed Image Text:5) Using values from Appendix C, calculate the standard enthalpy change for each
of the following reactions:
(a) 2 SO2(g) + O2(8)
2 SO3(8)
(b) Mg(OH)2(s)
MgO(s) + H2O(1)
(c) N2O4(8) + 4 H2(g)
→ N2(8) + 4 H2O(g)
(d) SiCl4(1) + 2 H2O(I)
SiO2(s) + 4 HCl(8)
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