Atkins’ Physical Chemistry Eighth Edition Chapter 2 – Lecture 4 The First Law Copyright © 2006...
Transcript of Atkins’ Physical Chemistry Eighth Edition Chapter 2 – Lecture 4 The First Law Copyright © 2006...
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Atkins’ Physical ChemistryEighth Edition
Chapter 2 – Lecture 4The First Law
Copyright © 2006 by Peter Atkins and Julio de Paula
Peter Atkins • Julio de Paula
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State Functions and Exact Differentials
• State function – state of the system independent of mannerand time to prepare
• Path functions – processes that describe prep of the state
• e.g., Heat, work, temperature
• Systems do not possess heat, work, or temperature
• Advantage of state functions:
• Can combine measurements of different properties toobtain value of desired property
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Fig 2.20 As V and T change, the internal energy, U changes
adiabatic
non-adiabatic
f
i
dUUΔ
When the systemcompletes the path:
dU is said to be:an exact differential
f
path,i
dqq
q is said to be:an inexact differential
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Fig 2.21 The partial derivative (∂U/∂V)T is the slope of Uw.r.t V at constant T
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Fig 2.22 The partial derivative (∂U/∂T)V is the slope of Uw.r.t T at constant V
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Fig 2.23 The overall change in U (i.e. dU) which arises whenboth V and T change
dTT
UdV
V
UdU
VT
The full differential of Uw.r.t V and T
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Partial derivatives representing physical properties:
VV T
UC
PP T
HC
Constant volume heat capacity
Constant pressure heat capacity
Internal pressureT
T V
U
π
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Fig 2.24 The internal pressure πT is the slope of U w.r.t. Vat constant T
has dimensions of pressure
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Partial derivatives representing physical properties:
VV T
UC
PP T
HC
Constant volume heat capacity
Constant pressure heat capacity
Internal pressureT
T V
U
π
dTCdVdTT
UdV
V
UdU VT
VT
πNow:
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Two cases for real gases:
0V
U
TT
π
Fig 2.25 For a perfect gas the internal energy is independentof volume at constant temperature
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Fig 2.26 Schematic of Joule’s attempt to measure ΔU foran isothermal expansion of a gas
TT V
U
π
at 22 atm
q absorbed by gas ∝ T
• For expansion into vacuum, w = 0
• No ΔT was observed,so q = 0
• In fact, experiment was crudeand did not detect thesmall ΔT
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Changes in Internal Energy at Constant Pressure
• Partial derivatives useful to obtain a property that cannotbe observed directly:
• e.g.,
• Dividing through by dT:
• Where expansion coefficient
• and isothermal compressibility
dTCdVdU VT π
VP
TP
CT
V
T
U
π
PT
V
V
1
α
TT P
V
V
1
κ
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VP
TP
CT
V
T
U
π
Changes in Internal Energy at Constant Pressure
VTP
CVT
U
απ
PT
V
V
1
α
TT P
V
V
1
κ
Substituting:
Into:
Gives:
For a perfect gas: VP
CT
U
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Changes in Internal Energy at Constant Pressure
• May also express the difference in heat capacities with observables:
• Cp – Cv = nR
• Since H = U + PV = U + nRT
• And:
PPVP T
U
T
HCC
nRT
HnR
T
UCC
PPVP
T
2
VPTV
CCκ
α