nsider 2.0 moles of methane (CH4 ), initially at 273 K, that is reversibly and adiabatically compressed from an initial volume of 10.00 L to a final volume of 2.00 L. 3a. Determine the final temperature, considering the gas to be described by the ideal gas equation of state. 3b. Determine the work required w, the associated heat flow q, and the internal energy change ∆U for the gas between the initial and final states.
nsider 2.0 moles of methane (CH4 ), initially at 273 K, that is reversibly and adiabatically compressed from an initial volume of 10.00 L to a final volume of 2.00 L. 3a. Determine the final temperature, considering the gas to be described by the ideal gas equation of state. 3b. Determine the work required w, the associated heat flow q, and the internal energy change ∆U for the gas between the initial and final states.
nsider 2.0 moles of methane (CH4 ), initially at 273 K, that is reversibly and adiabatically compressed from an initial volume of 10.00 L to a final volume of 2.00 L. 3a. Determine the final temperature, considering the gas to be described by the ideal gas equation of state. 3b. Determine the work required w, the associated heat flow q, and the internal energy change ∆U for the gas between the initial and final states.
Now, consider 2.0 moles of methane (CH4 ), initially at 273 K, that is reversibly and adiabatically compressed from an initial volume of 10.00 L to a final volume of 2.00 L.
3a. Determine the final temperature, considering the gas to be described by the ideal gas equation of state.
3b. Determine the work required w, the associated heat flow q, and the internal energy change ∆U for the gas between the initial and final states.
Transcribed Image Text:Integrals
r'dx
;n -1
n+1
Inx
-dx
ax -b
-In(ax - b)
=
Nomenclature – but, when in doubt, write it out!
AG Change in Gibbs free energy for an arbitrary process (energy)
AGm Change in Gibbs free energy for an arbitrary process, per mole (energy/mole)
AGn Molar Gibbs free energy change of chemical equation = (@G/Ə5)r.p (energy/mole)
AGan Standard Gibbs free change of chemical equation, per mole, between separated products and reactants, each in
the standard states for the phases specified. (energy/mole)
van der Waals equation of state
RT
an
V - nb
Virial equation of state
RT
p=
Vm
B
1+
+...
Vn V
Fundamental equations of thermodynamics
(constant composition)
Maxwell relations
(),--),
- (4),--),
(), --(#),
- (),--4),
From dU :
dU = TdS - pdv
av
as
TdS+V dp
-SdT – pdV
dA
From dH :
+
=+
se
P
dG
= -SdT +V dp
From dA:
+
as
From dG:
= +
Transcribed Image Text:Useful info
This and the following page contain physical constants, unit conversions, and chemical reference data that will be
essential to several of the problems on the exam. You may separate them from your exam for convenience, and they
do not need to be submitted with your answers.
NA =6.022×10 mol?
g = 9.807 m/s
Pm[H,O] =1.00 g/mL
1 bar = 10° Pa
1 atm =1.013bar
R = 8.314 J/K-mol
= 8.206x10 L-atm/K-mol
= 8.206x10° m-atm/K-mol
= 760 Torr
1 mbar = 10 bar
= 62.36 L-Torm/K-mol
1J = 10² L-bar = 9.870×10° L-atm= 0.2390 cal
1m = 10° cm = 10° mm = 10° µum = 10° nm = 1010 A
1 L-atm = 101.3 J
1 m = 10° L = 10° cm
1 kg = 1000 g
1 Watt (W) = 1 J/s
1 Volt (V) = 1 J/Coulomb
1 Coulomb (C) = 6.24 x 1018 elementary charges
F = 9.645 x 10 C/mol
At 298 K (only):
RT = 2.478 kJ/mol (= 24.46 L-atm/mol)
RT/F = 0.0257 V (= 25.7 mV)
Physical Properties of Selected Substances
mol. wt.
AH
Cp.m
AH
kJ/mol
melting temp AHap
kJ/mol
boiling temp
3,m
"fus
g/mol
44.0
kJ/mol
J/(mol-K) J/(mol-K)
K
K
CO,(g)
CH,(g)
CH,OH(I)
CH,OH(g)
n-C,H4()
H,(g)
H,O(1)
H,O(g)
Hg(1)
1,(8)
L(g)
HI(g)
O,(g)
Properties of pure phases are for standard conditions of 298 K and I atm.
Phase transition enthalpies are valid at the indicated phase transition temperature, at 1 atm.
-393.5
37.1
16.04
-74.8
35.3
0.94
91
8.2
112
32.04
-238.66
81.6
3.16
175.2
35.29
337.2
32.04
-200.66
43.9
86.2
-198.7
204.3
13.1
178
28.9
342
2.0
116.1
28.8
18.0
-285.8
69.9
75.3
6.0
273.15
40.6
373.15
18.0
-241.8
188.8
33.6
200.6
76.0
2.3
234.3
59.3
629.7
253.8
116.14
54.4
15.5
386.8
41.8
458.4
253.8
+62.44
260.69
36.9
127.91
+26.48
206.6
29.2
32.0
205.1
29.4
Branch of chemistry that studies how atoms, molecules, and materials interact with each other. Physical chemistry focuses on the behavior of matter, such as solids, liquids, and gases, as they interact with other matter. The study of physical chemistry is crucial to thermodynamics, quantum mechanics, and photochemistry.
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![Useful info
This and the following page contain physical constants, unit conversions, and chemical reference data that will be
essential to several of the problems on the exam. You may separate them from your exam for convenience, and they
do not need to be submitted with your answers.
NA =6.022×10 mol?
g = 9.807 m/s
Pm[H,O] =1.00 g/mL
1 bar = 10° Pa
1 atm =1.013bar
R = 8.314 J/K-mol
= 8.206x10 L-atm/K-mol
= 8.206x10° m-atm/K-mol
= 760 Torr
1 mbar = 10 bar
= 62.36 L-Torm/K-mol
1J = 10² L-bar = 9.870×10° L-atm= 0.2390 cal
1m = 10° cm = 10° mm = 10° µum = 10° nm = 1010 A
1 L-atm = 101.3 J
1 m = 10° L = 10° cm
1 kg = 1000 g
1 Watt (W) = 1 J/s
1 Volt (V) = 1 J/Coulomb
1 Coulomb (C) = 6.24 x 1018 elementary charges
F = 9.645 x 10 C/mol
At 298 K (only):
RT = 2.478 kJ/mol (= 24.46 L-atm/mol)
RT/F = 0.0257 V (= 25.7 mV)
Physical Properties of Selected Substances
mol. wt.
AH
Cp.m
AH
kJ/mol
melting temp AHap
kJ/mol
boiling temp
3,m
"fus
g/mol
44.0
kJ/mol
J/(mol-K) J/(mol-K)
K
K
CO,(g)
CH,(g)
CH,OH(I)
CH,OH(g)
n-C,H4()
H,(g)
H,O(1)
H,O(g)
Hg(1)
1,(8)
L(g)
HI(g)
O,(g)
Properties of pure phases are for standard conditions of 298 K and I atm.
Phase transition enthalpies are valid at the indicated phase transition temperature, at 1 atm.
-393.5
37.1
16.04
-74.8
35.3
0.94
91
8.2
112
32.04
-238.66
81.6
3.16
175.2
35.29
337.2
32.04
-200.66
43.9
86.2
-198.7
204.3
13.1
178
28.9
342
2.0
116.1
28.8
18.0
-285.8
69.9
75.3
6.0
273.15
40.6
373.15
18.0
-241.8
188.8
33.6
200.6
76.0
2.3
234.3
59.3
629.7
253.8
116.14
54.4
15.5
386.8
41.8
458.4
253.8
+62.44
260.69
36.9
127.91
+26.48
206.6
29.2
32.0
205.1
29.4](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3bf220d8-72cf-4063-a72c-68c9bd2e9a6e%2Ff94e97a1-384d-4396-838d-3619f462e38d%2Fvosb4ma_processed.png&w=3840&q=75)
