P Chem Flashcards

1
Q

Bohr Atom Energy

A

En = 13.6 eV / n^2

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2
Q

Nodes

A

Total: n - 1
Radial: n - l - 1
Angular: l

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3
Q

First Law of Thermodynamics

A

dU = q + w

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4
Q

Cp/Cv relationship

A

Cp - Cv = nR

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5
Q

PV work with Pext

A

w = -P(ext) (Vf - Vi)

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6
Q

Solving 1st Law for Q

A

q = dU - w = dU + P(ext)dV

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7
Q

Irreversible process work

A

w = - nRT ln(V2/V1)

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8
Q

Internal Energy with C

A

dU = qv = Cv(Tf - Ti)

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9
Q

Enthalpy/Interal Energy relationship

A

H = U + PV = U + nRT

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10
Q

Enthalpy with C

A

dH = qp = Cp(Tf-Ti)

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11
Q

Carnot efficiency

A

e = 1 - Tcold/Thot

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12
Q

Entropy, general

A

dS = nR ln(Vf/Vi) = -nR ln(Pf/Pi)

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13
Q

Entropy at constant V

A

dS = n Cv,m ln(Tf/Ti)

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14
Q

Entropy at constant P

A

dS = n Cp,m ln(Tf/Ti)

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15
Q

Entropy at phase change

A

dS = dHvap / dTvap (or fus)

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16
Q

Total entropy

A

dS(total) = dS + dS(surroundings)

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17
Q

Second Law of Thermodynamics

A

The entropy of an isolated system never decreases

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18
Q

Third Law of Thermodynamics

A

The entropy of a pure, perfectly crystalline substance is zero at zero kelvin

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19
Q

Absolute entropy

A

S = k ln (W)

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20
Q

DOF nonlinear gas molecule

A

3 Translational
3 Rotational
3n - 6 Vibrational

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21
Q

DOF linear gas molecule

A

3 Translational
2 Rotational
3n - 5 Vibrational

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22
Q

The entropy of all substances is a…

A

monotonically increasing function of temperature

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23
Q

Helmholtz Free Energy

A

A = U - TS

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24
Q

Gibbs Free Energy

A
G = H - TS
G = U + PV - TS
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25
dU
dU = TdS - PdV
26
dH
dH = TdS + VdP
27
dA
dA = -SdT - PdV
28
dG
dG = -SdT + VdP
29
Isobaric volumetric thermal expansion coefficient
a or b = (1/V) (dV/dT)_P
30
Isothermal compressibility
k = -(1/V)(dV/dP)_T
31
Gibbs-Helmholtz Equation
[d(G/T)/dT]_P = -H/T^2
32
dS(mixing)
dS(mixing) = -nR sum(xi ln(xi))
33
dG(R)
dG(R) = dG(R0) + RT ln Q
34
G/K relationship
dG = -RT ln K
35
K/T dependence
ln K@Tf = ln K@T0 - (dH/R)(1/Tf - 1/T0)
36
Error in IDG
z = Vm/Vm(ideal) = PVm/RT
37
Boyle temperature
Tb = a/Rb
38
An increase in P always leads to...
a boiling point elevation
39
Freezing point is elevated with increased P if...
V liq > V solid
40
Freezing point is depressed with increased P if...
V liq < V solid
41
dH(sublimation)
dH(sub) = dH(fus) + dH(vap)
42
Gibbs's Phase Rule for pure system
DOF = 3 - p
43
Clapeyron Equation
dP/dT = dSm/dVm | Slope of coexistence curve!
44
Trouton's Rule
dSm(vap) ~ 90 J/mol*K for liquids
45
Clausius-Clapeyron Equation
ln(Pf/Pi) = -(dHm(vap)/R) (1/Tf - 1/Ti)
46
Raoult's Law
Pi = xi Pi*
47
DOF for system with C components
DOF = C - p + 2
48
Gibbs-Duhem equations
n1dmu1 + n2dmu2 = 0 x1dmu1 + x2dmu2 = 0 x1dV1 + x2dV2 = 0
49
Boiling Point Elevation
dT(boiling) = Kb*molality(solute)
50
Freezing Point Depression
dT(freezing) = - Kf*molality(solute)
51
van't Hoff Equation
pi = n(solute)RT/V
52
Ideal Solution characterized by...
dGmix < 0 dSmix > 0 dV mix = 0 dH mix = 0
53
Henry's Law for solute
Pi = xi kHi as xi --> 0
54
Positive Deviation from Raoult's Law
A-B interactions are least attractive Minimum boiling azeotrope formed kH > Pi*
55
Negative Deviation from Raoult's Law
A-B interactions are most attractive Maximum boiling azeotrope formed kH < Pi*
56
Standard Solvent State
as xi --> 1, ai = Pi/Pi* gi = ai/xi
57
Standard Solute State
as xi --> 0, ai = Pi/kHi gi = ai/xi
58
G/E relationship
dG = -nfE
59
E/K relationship
E = (RT/nF) ln K
60
pH/pKa relationship
pH = pKa + log([A-]/[HA])
61
Vibrational states...
are only significantly populated at high T
62
Rotational states...
are populated at room T
63
rate k/Ea relationship
ln(k) = -Ea/RT
64
3 amino acids that have an isoelectric point not the average of their two lowest pKa's
Arg, His, Lys | + charged side chains
65
U(translation)
UT = (3/2)nRT
66
U(rotation)
``` UR = nRT (linear polyatomic) UR = (3/2)nRT (nonlinear polyatomic) ```
67
U(vibration)
UV = nRT in high T limit
68
U(electronic)
UE = 0
69
Dulong & Petit Law
Limiting value of heat capacity of a solid is 3R at high T
70
Debye modification to Einstein solids
Low T heat capacity is proportional to T^3