Overview Flashcards
(104 cards)
1
Q
Equation for percent composition by mass:
A
mass of solute/ mass of solution x 100
2
Q
Equation for mole fraction:
A
X = # of mol of compound / total # of moles in system
3
Q
Equation for molarity:
A
M = moles of solute / liters of solution
4
Q
Equation for molality:
A
m = moles of solute / kg of solvent
5
Q
Equation for gram equivalent weight:
A
GEW = molar mass / n
6
Q
Equation for normality:
A
N = # of gram equivalent weights of solute / liters of solution
7
Q
Equation for Keq:
A
[C]^c[D]^d/[A]^a[B]^b
8
Q
Equation for first law of thermodynamics:
A
deltaU = Q - W deltaU = change in internal energy Q = heat added to the system W = work done by the system
9
Q
Equation for ideal gas law:
A
PV = nRT P = pressure V = volume n= # of moles R = gas constant T = temp in kelvins
10
Q
Equation for density
A
p = m/V m = mass V = volume
11
Q
Equation for Boyle’s Law:
A
P1V1 = P2V2
12
Q
Equation for Charles’s Law:
A
V1/T1 = V2/T2
13
Q
Equation for Gay-Lussac’s Law:
A
P1/T1 = P2/T2
14
Q
Equation for combined gas law:
A
P1V1/T1 = P2V2/T2
15
Q
Equation for Avogadro’s Principle:
A
n1/V1 = n2/V2
16
Q
Equation for Henry’s Law:
A
[A]1/P1 = [A]2/P2 = Kh [A] = conc of A in solution Kh = Henry's constant PA = partial pressure of A
17
Q
Equation for Graham’s Law of Diffusion and Effusion:
A
r1/r2 = sqrt(M1/M2) r1/r2 = diffusion of gas 1 and 2 M1/M2 = molar mass
18
Q
Equation for Van der Waals Equation of state:
A
(P + n^2*a/V^2)(V - nb) = nRT P = pressure a/b = physical constants experimentally determines for a gas a = corrects for attractive forces b = corrects for volume of particles n = # of moles
19
Q
What is the variable for enthalpy?
A
H
20
Q
What is enthalpy?
A
equal to the heat transferred into or out of the system at constant P
21
Q
Equation for enthalpy of a reaction:
A
deltaHrxn = Hproducts - Hreactants
22
Q
What is the standard heat of formation?
A
the enthalpy required to produce one mole of a compound from its elements in their standard states
23
Q
What is the standard heat of reaction?
A
enthalpy change accompanying a reaction being carried out under standard conditions
24
Q
Equation for standard heat of reaction:
A
deltaHrxn = Sum(deltaHf, products) - Sum(deltaHf, reactants)
25
Equation for Hess's Law:
DeltaH = DeltaH1 + DeltaH2 + DeltaH3
26
Equation for bond dissociation energies
DeltaHrxn = Sum(Deltabondsbroken) - Sum(Deltabondsformed)
27
What is the variable for entropy?
S
28
What is entropy?
measure of spontaneous dispersal of energy at a specific temperature
29
Equation for entropy:
deltaS = Qrev / T
| Qrev - heat gained or lost in a reversible reaction
30
What is the solubility product constant?
Ksp - dissolution of the original solution
31
What is the stability/formation constant?
Kf - subsequent formation of the complex ion in solution
32
Equation for Raoult's Law:
```
Pa = Xa*Pa^o
Pa = vapor pressure of solvent A when the solutes are present
Xa = mole fraction of solvent A in the solution
Pa^o = vapor pressure of solvent A in its pure state
```
33
Equation for boiling point elevation:
```
deltaTb = i*Kb*m
deltaTb = increase in boiling point
i = # of particles into which a compound dissociated in solution
Kb = proportionality constant characteristic of a particular solvent
m = molality
```
34
Equation for freezing point depression:
```
deltaTf = i*Kf*m
deltaTb = decrease in freezing point
i = # of particles into which a compound dissociates in solution
Kf = proportionality constant characteristic of a particular solvent
m = molality
```
35
Equation for osmotic pressure:
```
pi = iMRT
pi = osmotic pressure
i = # of particles into which a compound dissociates in solution
M = molarity
R = ideal gas constant
T = temp in kelvins
```
36
Henderson-Hasselbalch equation:
pH = pKa + log[A-]/[HA]
37
Relationship between pH and hydroniums ions:
pH = -log[H+]
38
Equation for acid dissociation constant:
Ka = [H3O+][A-]/[HA]
39
Relationship between pKa and Ka:
pKa = -logKa
40
Equation and value for water dissociation constant:
Kw = [H3O+][OH-] = 10^-14
41
Variable for free energy:
G
42
Equation for Gibbs free energy:
```
deltaG = deltaH - T*deltaS
deltaG = change in free energy
deltaH = change in enthalpy
T = temp in K
deltaS = change in entropy
```
43
Equation for standard free energy:
```
deltaG^orxn = -R*T*lnKeq
deltaG^orxn = change in standard free energy
R = ideal gas constant
T = temp in kelvins
Keq = equilibrium constant
```
44
Equation for change in free energy under nonstandard conditions:
deltaGrxn = deltaG^orxn + R*T*lnQ
45
Equation for Gibbs free energy in relation to emf:
```
deltaG^o = -nFE^ocell
deltaG^o = standard free energy
n = # of moles of e- exchanged
F = Faraday's constant
E^ocell = standard emf of the cell
```
46
Nernst equation:
```
Ecell = E^ocell - (RT/nF)*lnQ
Ecell = emf of cell under nonstandard conditions
E^ocell = emf of the cell under standard conditions
R = ideal gas constant
T = temp in kelvins
F = faradays constant
Q = reaction quotient for the reaction at a given point in time
```
47
Equation for standard electromotive force:
E^ocell = Ered, cathode - Ered, anode
48
What is faraday's constant and units?
10^-5 C/mol*e-
49
Equation for heat released/absorbed in a process:
```
q = mcdeltaT
q = heat
m = mass
c = specific heat of the substance
deltaT = change in temp
```
50
What is the ideal gas constant and units?
R = 8.3145 J/mol*K
51
Equation for percent yield:
% yield = actual yield/theoretical yield x 100%
52
Avogadro's number and units:
6.022 x 10^23 mol^-1
53
Entropy units:
J/mol*K
54
1 calorie = ______ J
4,184 J
55
Specific heat of water:
1 cal/g*K
56
How do Kw, Ka and Kb relate?
Kw = Ka * Kb
57
Electrodeposition equation:
```
molM = I*t/n*F
molM = amount of metal ion being deposited at a specific electrode
I = current
t = time
n = # of e- equivalents for a specific metal ion
F = faraday's constant
```
58
What is oxidation?
loss of electrons
59
What is reduction?
gain of electrons
60
What is an oxidizing agent?
causes oxidation (loss e-) and becomes reduced itself (gain e-)
61
What is a reducing agent?
causes reduction (gain e-) and becomes oxidized itself (loss e-)
62
In electrochemical cells, oxidation happens at the _____.
anode
63
In electrochemical cells, reduction happens at the ______.
cathode
64
In galvanic cells, the cathode has a _____ reduction potential.
more positive
65
In galvanic cells, the anode has a _____ reduction potential.
less positive
66
In electrolytic cells, the cathode has a _____ reduction potential.
less positive
67
In electrolytic cells, the anode has a _____ reduction potential.
more positive
68
If the emf is positive, the cell _____ energy.
releases
69
If the emf is negative(?), the cell _____ energy.
absorbs
70
Electrons move from _____ to ______ in electrochemical cells.
anode to the cathode
71
Current moves from _____ to _____ in electrochemical cells.
cathode to anode
72
Definition of an Arrhenius acid
dissociate to form an excess of H+ in solution
73
Definition of an Arrhenius base
dissociate to form an excess of -OH in solution
74
Definition of a Bronsted-Lowry acid
a species that donates H+ ions
75
Definition of a Bronsted-Lowry base
a species that accepts H+ ions
76
Definition of a Lewis acid
electron pair acceptor
77
Definition of a Lewis base
electron pair donor
78
A _____ acid and _____ base will have an equivalence point < 7.
strong; weak
79
A _____ acid and _____ base will have an equivalence point = 7.
strong;strong
80
A _____ acid and _____ base will have an equivalence point > 7.
weak;strong
81
Ammonium is soluble or insoluble in water?
soluble
82
Alkali metals soluble or insoluble in water?
soluble
83
Nitrate salts soluble or insoluble in water?
soluble
84
Acetate salts soluble or insoluble in water?
soluble
85
Cl-,Br-, and I- are soluble/insoluble in water with exceptions of ______.
soluble; Ag+, Pb2+,Hg22+
86
Sulfate are soluble/insoluble in water with exceptions of ______.
soluble; Ca2+, Sr2+, Ba2+, Pb2+
87
Metal oxides are soluble/insoluble in water with exceptions of ______.
insoluble; alkali metals, NH4+, CaO, SrO, BaO
88
Hydroxides are soluble/insoluble in water with exceptions of ______.
insoluble; alkali metals, NH4+, Ca2+, Sr2+, Ba2+
89
Carbonates are soluble/insoluble in water with exceptions of ______.
insoluble; alkali metals, NH4+
90
Phosphates is soluble or insoluble in water?
insoluble
91
Sulfides is soluble or insoluble in water?
insoluble
92
Sulfites is soluble or insoluble in water?
insoluble
93
Equation for how much heat is needed to move from one phase to another and no change in temp:
```
q = mL
q = heat
m = mass
L = latent heat/enthalpy of an isothermal process (g/cal)
```
94
Name of a process with constant heat:
adiabatic process
95
Name of a process with constant internal energy:
isothermal process
96
Name of a process with constant pressure:
isobaric process
97
Name of a process with constant volume:
isovolumetric/isochoric process
98
What are the standard conditions?
298K (25C)
1 atm
1 M conc
99
What is STP?
273K (0C)
| 1 atm
100
What is standard conditions used for?
kinetics, equilibrium, thermodynamics
101
What is STP used for?
ideal gas calculations
102
Name 8 state functions:
```
Pressure
Density
Temperature
Volume
Enthalpy
Internal energy
Gibbs free energy
Entropy
```
103
What is solid to gas phase called?
sublimation
104
What is gas to solid phase called?
deposition
