1 phase equilibria (ch-203) phase transitions change in phase without a change in chemical...
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Phase Equilibria (CH-203)
Phase transitions Change in phase without a change in chemical composition
Gibbs energy is at the centre of the discussion of transitions
Molar Gibbs energyGm = G/n = H - TS
Depends on the phase of the substance
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A substance has a spontaneous tendency to change into a phase with the lowest
molar Gibbs energy
When an amount n of a substance changes from phase 1 (e.g. liquid) with molar Gibbs energy Gm(1) to phase 2 (e.g. vapour) with molar Gibbs energy Gm(2), the change in Gibbs energy is:
G = nGm(2) – nGm(1) = n{Gm(2) – Gm(1)}
A spontaneous change occurs when G < 0
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The Gibbs energy of transition from metallic white tin (-Sn) to nometallic grey tin (-Sn) is +0.13 kJ mol-1 at 298 K. Which is the reference state of tin at this temperature?
White tin!
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If at a certain temperature and pressure the solid phase of a substance has a lower molar Gibbs energy than its liquid phase, then the solid phase will be thermodynamically more stable and the liquid will (or at least have a tendency) to freeze.
If the opposite is true, the liquid phase is thermodynamically more stable and the solid will melt.
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Proof-go back to fundamental definitions
G = H – TS; H = U + pV; U = q + wFor an infinitesimal change in G:
G + G = H + H – (T + T)(S + S) = H + H – TS – ST – TS – TSG = H – TS – STAlso can write: H = U + pV + Vp
U = TS – pV (dS = dqrev/T and dw = -pdV)
G = TS – pV + pV +Vp – TS – ST
G = Vp – ST Master Equations
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Variation with pressure
Thus, Gibbs energy depends on:– Pressure– Temperature
We can derive (derivation 5.1 in textbook) that:
Gm = Vm p
=>Gm > 0 when p > 0
i.e. Molar Gibbs energy increases when pressure increases
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Variation of G with pressure
Can usually ignore pressure dependence of G for condensed states
Can derive that, for a gas:
i
fm p
pRTG ln
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Variation of G with temperature
Gm = –SmT
Gm= Gm(Tf) – Gm(Ti)
T = Tf – Ti
Can help us to understand why transitions occur
The transition temperature is the temperature when the molar Gibbs energy of the two phases are equal
The two phases are in EQUILIBIRIUM at this temperature
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Variation of G with temperature
Gm = –SmT
Molar entropy is positive, thus an increase in T results in a decrease in Gm. Because:
Gm Sm
more spatial disorder in gas phase than in condensed phase, so molar entropy of gas phase is larger than for condensed phase.
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Why do substances melt and vaporise?
At lower T solid has lowest Gm and thus most stable
As T increases, Gm of liquid phase falls below the solid phase and substance melts
At higher T, Gm of gas phase plunges below that of the liquid phase and the substance vaporises
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Substances which sublime (CO2)
There is no temperature at which the liquid phase has a lower Gm than the solid phase.
Thus, as T increases the compound eventually sublimes into the gas phase.
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Phase diagrams
Map showing conditions of T and p at which various phases are thermodynamically stable
At any point on the phase boundaries, the phases are in dynamic equilibrium
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Phase boundaries
The pressure of the vapour in equilibrium with its condensed phase is called the vapour pressure of the substance.– Vapour pressure increases with temperature
because, as the temperature is raised, more molecules have sufficient energy to leave their neighbours in the liquid.
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Vapour pressure of water versus T
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Phase boundaries
Suppose liquid in a cylinder fitted with a piston.
Apply pressure > vapour pressure of liquid– vapour eliminated– piston rests on surface of liquid– system moves to liquid region of phase diagram
Reducing pressure????????
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Question
What would be observed when a pressure of 7.0 kPa is applied to a sample of water in equilibrium with its vapour at 25oC, when its vapour pressure is 2.3 kPa?
Sample condenses entirely to liquid
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Solid-Solid phase boundaries
Thermal analysis:– uses heat release
during transition
Sample allowed to cool and T monitored
On transition, energy is released as heat and cooling stops until transition is complete
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Location of phase boundaries
Suppose two phases are in equilibrium at a given p and T.
If we change p, we must change T to a different value to ensure the two phases remain in equilibrium.
Thus, there must be a relationship between p that we exert and T we must make to ensure that the two phases remain in equilibrium
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Location of phase boundaries Clapeyron equation (see derivation 5.4)
Clausius-Clapeyron equation (derivation 5.5)
TVT
Hp
trs
trs
constant11
lnln
ln
1212
2
2
TTR
Hpp
TRT
Hp
TRT
H
p
p
vap
vap
vap
Constant is
vapS/R
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Example 1The vapour pressure of mercury is 160 mPa at 20°C. What is its vapour pressure at 50°C given that its enthalpy of vaporisation is 59.3 kJ mol-1?
Pa53.1
426096.0ln
258676.283258.1ln
)1016685.3(25.713283258.1ln
15.293
1
15.323
1
314.8
59300)10160ln(ln
constant11
lnln
2
2
2
42
32
1212
p
p
p
xp
xp
TTR
Hpp
vap
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Example 2The vapour pressure of pyridine is 50.0 kPa at 365.7 K and the normal boiling point is 388.4 K. What is the enthalpy of vaporisation of pyridine?
1
5
4
1212
molkJ74.36
10922258.1
7063.0
)10598165.1(314.8
7063.0
7.365
1
4.388
1
314.850000
101325ln
constant11
lnln
H
Hx
xH
H
TTR
Hpp
vap
vap
vap
vap
vap
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Example 3Estimate the boiling point of benzene given that its vapour pressure is 20.0 kPa at 35°C and 50.0 kPa at 58.8°C?
1
5
4
1212
molkJ74.32
1079854.2
91629.0
)10326709.2(314.8
91629.0
95.331
1
15.308
1
314.850000
20000ln
constant11
lnln
H
Hx
xH
H
TTR
Hpp
vap
vap
vap
vap
vap
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Example 3 contd.
KT
Tx
xT
x
T
T
TTR
Hpp
vap
353
/110833193.2
1024517.31
1011977.4
15.308
1157.39386226.1
15.308
11
314.8
2.32745
20000
101325ln
constant11
lnln
2
23
3
2
4
2
2
1212
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Vapour pressure
)log10ln(ln
10ln
10lnln
log
constant11
lnln
'
'
1212
yxy
R
HB
RT
H
kPa
PA
T
BAp
TTR
Hpp
vap
vap
vap
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Vapour pressure
Substance A B/K Temperature range/°C
Benzene, C6H6(l) 7.0871 1785 0 to 42
6.7795 1687 42 to 100
Hexane, C6H14(l) 6.849 1655 10 to 90
Methanol, CH3OH(l) 7.927 2002 10 to 80
Methylbenzene, C6H5CH3(l) 7.455 2047 92 to 15
Phosphorus, P4(s, white) 8.776 3297 20 to 44
Sulfur trioxide, SO3(l) 9.147 2269 24 to 48
Tetrachloromethane, CCl4(l) 7.129 1771 19 to 20
* A and B are the constants in the expression log(p/kPa) A B/T.
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The vapour pressure of benzene in the range 042 oC can be expressed in the form log (p/kPa) = 7.0871 1785 K/ T. What is the enthalpy of vaporisation of liquid benzene?
1molkJ17.34
10ln3145.8178510ln
)kPa/( log
H
HxxR
HB
T
BAp
vap
vap
vap
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For benzene in the range 42100oC, B = 1687 K and A = 6.7795. Estimate the normal boiling point of benzene?
K38.353
16877796.60057.2
16877796.6)325.101log(
)kPa/( log
TT
T
T
BAp
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Derivations
dGm = Vmdp – SmdTdGm(1) = dGm(2)
Vm(1)dp – Sm(1)dT = Vm(2)dp – Sm(2)dT
{Vm(2) – Vm(1)}dp = {Sm(2) – Sm(1)}dT
trsV dp = trsS dT
T trsV dp = trsH dT
dp/dT = trsH/(T trsV)
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Derivations: liquid-vapour transitions
dp/dT = vapH/(T vapV)
≈ vapH/{T Vm(g)} = vapH/{T (RT/p)}
(dp/p)/dT = vapH/(RT2)
d(ln p)/dT = vapH/(RT2)
122
1
2
2
ln
ln
2
111ln
ln
ln
2
1
2
1
2
1
TTR
HdT
TR
H
p
p
dTRT
Hpd
dTRT
Hpd
vapT
T
vap
T
T
vapp
p
vap
+ constant
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Heat liquid in open vessel
As T is raised the vapour pressure increase.
At a certain T, the vapour pressure becomes
equal to the external pressure.
At this T, the vapour can drive back the
surrounding atmosphere, with no constraint on
expansion, bubbles form an boiling occurs.
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Characteristic points
Remember: BP: temperature at which the vapour
pressure of the liquid is equal to the prevailing atmospheric pressure.
At 1 atm pressure: Normal Boiling Point (100°C for water)
At 1 bar pressure: Standard Boiling Point (99.6°C for water; 1 bar = 0.987atm, 1 atm = 1.01325 bar)
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Heat liquid in closed vessel Vapour density increases until it equals that of
the liquid– surface between the two layers disappears– T is known as the critical temperature (TC)– vapour pressure at TC is critical pressure pC
– TC and pC together define the critical point If we exert pressure on a sample that is above
TC we produce a denser fluid No separation, single uniform phase of a
supercritical fluid occupies the container
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Heat liquid in closed vessel
A liquid cannot be produced by the application of pressure to a substance if it is at or above its critical temperature
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Triple point
There is a set of conditions under which three different phases coexist in equilibrium. The triple point. For water the triple point lies at 273.16 K and 611 Pa (0.006 atm).
The triple point marks the lowest T at which the liquid can exist
The critical point marks the highest T at which the liquid can exist
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Summary• Thermodynamics tells which way a process will go
• Internal energy of an isolated system is constant (work
and heat). We looked at expansion work (reversible and
irreversible).
• Thermochemistry usually deals with heat at constant
pressure, which is the enthalpy.
• Spontaneous processes are accompanied by an increase
in the entropy (disorder?) of the universe
• Gibbs free energy decreases in a spontaneous process