please answer all the following: How much energy per mole does it take to boil each of the following molecules from starting at standard state ambient temperature, 298 K. Boiling means increase temperature to the boiling point and then converting the liquid to a gas. Assume constant pressure conditions. Use Table 2C.1 to find Tboil and ΔHvap. Use Table 2C.7 to find Cpm values. a. Methanol (CH3OH) b. Ethanol (C2H5OH) c. Water (H2O) d. Which needs the largest amount of energy? What factor has the greater impact on this value?
please answer all the following: How much energy per mole does it take to boil each of the following molecules from starting at standard state ambient temperature, 298 K. Boiling means increase temperature to the boiling point and then converting the liquid to a gas. Assume constant pressure conditions. Use Table 2C.1 to find Tboil and ΔHvap. Use Table 2C.7 to find Cpm values. a. Methanol (CH3OH) b. Ethanol (C2H5OH) c. Water (H2O) d. Which needs the largest amount of energy? What factor has the greater impact on this value?
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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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
please answer all the following:
How much energy per mole does it take to boil each of the following molecules from starting at standard state ambient temperature, 298 K. Boiling means increase temperature to the boiling point and then converting the liquid to a gas. Assume constant pressure conditions. Use Table 2C.1 to find Tboil and ΔHvap. Use Table 2C.7 to find Cpm values.
a. Methanol (CH3OH)
b. Ethanol (C2H5OH)
c. Water (H2O)
d. Which needs the largest amount of energy? What factor has the greater impact on this value?
Transcribed Image Text:Table 2C.7 (Continued)
Caesium (cesium)
Cs(s)
Cs(g)
Cs'(aq)
Chlorine
Cl₂(g)
Cl(g)
Cl (g)
Cl(aq)
HCI(g)
HCl(aq)
M/(g mol)
Chromium
Cr(s)
Cr(g)
Cro (aq)
Cr,O, (aq)
132.91
132.91
132.91
Calcium
Ca(s)
Ca(g)
Ca³(aq)
CaO(s)
CaCO,(s) (calcite)
CaCO,(s) (aragonite)
CaF.(s)
CaCl₂(s)
CaBr(s)
Carbon (for 'organic' compounds of carbon, see Table 2C.6)
C(s) (graphite)
C(s) (diamond)
C(g)
C₂(g)
CO(g)
CO₂(g)
CO,(aq)
H,CO,(aq)
HCO; (aq)
CO(aq)
CCI (1)
CS,(1)
HCN(g)
HCN(1)
CN (aq)
40.08
40.08
40.08
56.08
100.09
100.09
78.08
110.99
199.90
12.011
12.011
12.011
24.022
28.011
44.010
44.010
62.03
61.02
60.01
153.82
76.14
27.03
27.03
26.02
70.91
35.45
34.45
35.45
36.46
36.46
A,H/(k) mol™¹)
52.00
52.00
115.99
215.99
0
+76.06
-258,28
0
+178.2
-542.83
-635.09
-1206.9
-1207.1
-1219.6
-795.8
-682.8
0
+1.895
+716.68
+831.90
-110.53
A-393.51
-413.80
-699.65
-691.99
-677.14
-135.44
+89.70
+135.1
+108.87
+150.6
0
+121.68
-233.13
-167.16
-92.31
-167.16
0
+396.6
-881.15
-1490.3
AG/(kJ mol)
C
0
+49.12
-292.02
0
+144.3
-553.58
-604.03
-1128,8
-1127.8
-1167.3
-748.1
-663.6
0
+2.900
+671.26
+775.89
-137.17
-394.36
-385.98
-623.08
3648-586.77
-527.81
-65.21
+65.27
+124.7
+124.97
+172.4
0
+105.68
-131.23
-95.30
-131.23
0
+351.8
-727.75
-1301.1
S/J K' mol')'
85.23
175.60
+133.05
41.42
154.88
-53.1
XOC
39.75
92.9
88.7
68.87
104.6
130
5.740
2.377
158.10
199.42
197.67
213.74
117.6
187.4
+91.2
-56.9
216.40
151.34
201.78
112.84
+94.1
223.07
165.20
+56.5
186.91
56.5
23.77
174.50
+-50.21
+261.9
CUK'mol)
32.17
20.79
-10.5
25.31
20,786
42.80
81.88
81.25
67.03
72.59
8.527
6.113
20.838
43.21
29.11
37.11
131.75
75.7
35.86
70.63
33.91
21.840
-136.4
29.12
-136.4
23.35
20.79
(sell
(Continued)
Transcribed Image Text:HD-
LLE
00
le 2C.7 (Continued)
Copper
Cu(s)
Cu(g)
Cu (aq)
Cu³(aq)
Cu₂O(s)
CuO(s)
CuSO,(s)
CuSO, H₂O(s)
CuSO,.5H₂O(s)
Deuterium
D₂(g)
HD(g)
D₂O(g)
D,O(1)
HDO(g)
HDO(1)
Fluorine
F₂(g)
F(g)
F'(aq)
HF(g)
Gold
Au(s)
Au(g)
Helium
He(g)
H₂(g)
H(g)
H*(aq)
H*(g)
H₂O(s)
H,O(1)
H₂O(g)
H₂O,(1)
lodine
I, (s)
L₂(g)
I(g)
l(aq)
HI(g)
M/(g mol"')
63.54
63.54
63.54
63.54
143.08
79.54
159.60
177.62
249.68
4.028
3.022
20.028
20.028
19.022
19.022
38.00
19.00
19.00
20.01
196.97
196.97
Hydrogen (see also deuterium)
14.003
MLAD
BL 2.016
1.008
1.008
1.008
18.015
18.015
18.015
34.015
253,81
253.81
126.90
126.90
127.91
to
AN
AH'/(kJ mol"')
0
+338.32
+71.67
+64.77
-168.6
-157.3
-771.36
-1085.8
-2279.7
ca
0
+0.318
-249.20
-294.60
-245.30
-289.89
0
+78.99
-332.63
-271.1
0
+366.1
0
0
+217.97
0
+1536.20
-285.83
-241.82
-187.78
0
+62.44
+106.84
-55.19
+26.48
4G/(kJ mol')
Libi
LEXIC
0
+298.58
+49.98
+65.49
-146.0
-129.7
-661.8
-918.11
-1879.7
0
-1.464
-234.54
-243.44
-233.11
-241.86
0
+61.91
-278.79
-273.2
0
+326.3
0
0
+203.25
0
21-237.13
-228.57
2-120.35
0
+19.33
+70.25
-51.57
+1.70
10
S/JK' mol')'
1511
LA
BIS
0
33.150
166.38
+40.6
-99.6
93.14
42.63
109
146.0
300.4
144.96
143.80
198.34
75.94
199.51
79.29
202.78
158.75
-13.8.
173.78
0
47.40
180.50
10126.15
SE 130.684
114.71
0
A
EB.OV-
69.91
188.83
109.6
0.02-116.135
260.69
180.79
+111.3
206.59
CUK'mol)
24.44
20.79
05.0
63.64
42.30
100.0
134
280
29.20
29.196
34.27
84.35
33.81
31.30
22.74
-106.7
29.13
ICM
25.42
20.79
20.786
28.824
20.784
0
37.99
75.291
33.58
89.1
254.44
36.90
20.786
-142.3
CIOR
29.158
TM
Expert Solution
Step 1
All three substances are liquid at 298 K.
moles of substance, n = 1 mol
#(a): Methanol:
The following data is required to solve the problem:
Boiling point of methanol = 337.85 K
Specific heat capacity of liquid methanol, C = 81.1 J.mol-1.K-1
Molar enthalpy of vaporization of liquid methanol, Hvap = 37.6 kJ/mol
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