Final exam Flashcards
Definition of pressure
P = F/A
Definition of work
dw= -PextdV
first law of thermo
dU = dQ + dw
definition of heat capacity
C = (∂Q/∂T)
What is U a function of?
T and V
Definition of enthalpy
H = U + PV
Heat capacity at a constant volume
Cv = (∂U/∂T)v
heat capactiy at a constant pressure
Cp = (∂H/∂T)p
Definition of entropy
ds = dQrev/T
Change in entropy for the irreversible isothermal expansion of an ideal gas
∆S = nRln(V2/V1) = -nRln(P2/P1)
Change in entropy for the heating of a gas from T1 to T2 keeping volume constant
∆S = Cv*ln(T2/T1)
Change in entropy for the heating of a gas from T1 to T2 keeping pressure constant
∆S = Cp*ln(T2/T1)
Entropy of mixing for an ideal gas
∆Smix = naRln(1/ya) + nbRln(1/yb)
na and nb are the number of moles and ya and yb are the mole fractions
Definition of G
G = H - TS
Defintion of A
A = U - TS
entropy of phase transitions
∆S = ∆H/T
(∂U/∂T)v = ?
Cv
(∂H/∂T)p = ?
Cp
T(∂S/∂T)v = ?
Cv
T(∂S/∂T)p = ?
Cp
(∂G/∂T)p = ?
-S
(∂A/∂T)v = ?
-S
(∂G/∂P)T = ?
V
(∂A/∂V)T = ?
-P
Gm = G/n = ?
µ
Basic equations
dU = Tds - PdV dA = -SdT -PdV dH = TdS + VdP dG = -SdT + VdP
Clausius Equation
dP/dT = ∆H / T∆V
Clausius- Clapeyron Equation
d(ln(P))/dT = ∆Hm/R(T^2)
Chemical potential of an ideal gas
µ = µ˚ + RTln(P/P˚)
Van’t Hoff equation
ln(Ka) = -∆H˚/RT+∆S/R
∆G = ? not at equilibrium when you have ∆G˚
∆G = ∆G˚ + RTln(Q)
∆G = ? not at equilibrium when you dont have ∆G˚
∆G = RTln(Q/Ka)
∆G˚ = ?
∆G˚ = -RTln(Ka)
Arrhenius Equation
K=A*exp(-Ea/RT)
gibbs phase rule
F = C - P + 2
F - DOF
C - # of the components
P - # of phases
Gibbs energy of mixing for an ideal solution
ntotal R T ∑xi ln(xi)
entropy of mixing for an ideal solution
R ∑ ni ln(xi)
