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CHEM1102 Thermodynamics Equations
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First Law
ΔE
sys
=
ΔEsys = q
p
+ w
(+ve is endo, -ve is exo)
Second Law
ΔS
uni
=
ΔSuni = ΔS
sys
+ ΔS
surround
Heat Capacity
q =
(include units)
q = C x ΔT
(in JK
-1
or JK
-1
g
-1
)
Calorimeter
w =
ΔE =
w = -P
ex
ΔV
ΔE = q
Heat (Enthalpy)
H =
ΔH =
H = E + PV
ΔH = q
p
(heat added to system)
Heat (Enthalpy)
ΔH
0
is
Δ
f
H
0
is
Δ
reaction
H
0
=
ΔH
0
is standard enthalpy (1 atm, 25
0
C)
Δ
f
H
0
is enthalpy of formation
Δ
reaction
H
0
= ΣnΔ
f
H
0
(products) - ΣnΔ
f
H
0
(reactants)
Entropy
Δ
reaction
S
0
=
Δ
reaction
S
0
= ΣnΔS
0
(products) - ΣnΔS
0
(reactants)
Entropy
ΔS
sys
=
ΔS
sys
= q
rev
JK
-1
mol
-1
(q is heat from T reversible change)
Entropy
ΔS
surround
=
ΔS
s
urround
=
heat transfer in actual process
T
=
-q
p
=
-ΔH
sys
T T
Gibb's Free Energy
G =
ΔG
sys
=
G = H - TS
ΔG
sys
= ΔH
sys
- TΔS
sys
at constant T
Gibb's Free Energy
Δ
reaction
G
0
=
Δ
reaction
G
0
= ΣnΔ
f
G
0
(products) - ΣnΔ
f
G
0
(reactants)
Equilibrium
ΔG
0
=
ΔG =
ΔG
0
= - RT lnK
ΔG = ΔG
0
+ RT lnQ
Spontaneity
Signs in Spontaneity
for G
sys
and S
uni
Signs in Equilibrium
G
sys
is -ve
S
uni
is +ve
In Equi, both are = 0
Author
Boost
ID
247899
Card Set
CHEM1102 Thermodynamics Equations
Description
CHEM1102 Thermodynamics Equations
Updated
2013-11-19T23:41:24Z
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