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General Chemistry > Overview > Flashcards

Overview Flashcards

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1
Q

Equation for percent composition by mass:

A

mass of solute/ mass of solution x 100

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2
Q

Equation for mole fraction:

A

X = # of mol of compound / total # of moles in system

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3
Q

Equation for molarity:

A

M = moles of solute / liters of solution

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4
Q

Equation for molality:

A

m = moles of solute / kg of solvent

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5
Q

Equation for gram equivalent weight:

A

GEW = molar mass / n

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6
Q

Equation for normality:

A

N = # of gram equivalent weights of solute / liters of solution

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7
Q

Equation for Keq:

A

[C]^c[D]^d/[A]^a[B]^b

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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
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9
Q

Equation for ideal gas law:

A 
PV = nRT
P = pressure
V = volume
n= # of moles
R = gas constant
T = temp in kelvins
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10
Q

Equation for density

A 
p = m/V
m = mass
V = volume
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11
Q

Equation for Boyle’s Law:

A

P1V1 = P2V2

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12
Q

Equation for Charles’s Law:

A

V1/T1 = V2/T2

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13
Q

Equation for Gay-Lussac’s Law:

A

P1/T1 = P2/T2

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14
Q

Equation for combined gas law:

A

P1V1/T1 = P2V2/T2

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15
Q

Equation for Avogadro’s Principle:

A

n1/V1 = n2/V2

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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
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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
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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
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19
Q

What is the variable for enthalpy?

A

H

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20
Q

What is enthalpy?

A

equal to the heat transferred into or out of the system at constant P

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21
Q

Equation for enthalpy of a reaction:

A

deltaHrxn = Hproducts - Hreactants

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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

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23
Q

What is the standard heat of reaction?

A

enthalpy change accompanying a reaction being carried out under standard conditions

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24
Q

Equation for standard heat of reaction:

A

deltaHrxn = Sum(deltaHf, products) - Sum(deltaHf, reactants)

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25
Q

Equation for Hess’s Law:

A

DeltaH = DeltaH1 + DeltaH2 + DeltaH3

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26
Q

Equation for bond dissociation energies

A

DeltaHrxn = Sum(Deltabondsbroken) - Sum(Deltabondsformed)

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27
Q

What is the variable for entropy?

A

S

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28
Q

What is entropy?

A

measure of spontaneous dispersal of energy at a specific temperature

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29
Q

Equation for entropy:

A

deltaS = Qrev / T

Qrev - heat gained or lost in a reversible reaction

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30
Q

What is the solubility product constant?

A

Ksp - dissolution of the original solution

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31
Q

What is the stability/formation constant?

A

Kf - subsequent formation of the complex ion in solution

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32
Q

Equation for Raoult’s Law:

A 
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
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33
Q

Equation for boiling point elevation:

A 
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
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34
Q

Equation for freezing point depression:

A 
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
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35
Q

Equation for osmotic pressure:

A 
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
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36
Q

Henderson-Hasselbalch equation:

A

pH = pKa + log[A-]/[HA]

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37
Q

Relationship between pH and hydroniums ions:

A

pH = -log[H+]

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38
Q

Equation for acid dissociation constant:

A

Ka = [H3O+][A-]/[HA]

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39
Q

Relationship between pKa and Ka:

A

pKa = -logKa

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40
Q

Equation and value for water dissociation constant:

A

Kw = [H3O+][OH-] = 10^-14

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41
Q

Variable for free energy:

A

G

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42
Q

Equation for Gibbs free energy:

A 
deltaG = deltaH - T*deltaS
deltaG = change in free energy
deltaH = change in enthalpy
T = temp in K
deltaS = change in entropy
43
Q

Equation for standard free energy:

A 
deltaG^orxn = -R*T*lnKeq
deltaG^orxn = change in standard free energy
R = ideal gas constant
T = temp in kelvins
Keq = equilibrium constant
44
Q

Equation for change in free energy under nonstandard conditions:

A

deltaGrxn = deltaG^orxn + RTlnQ

45
Q

Equation for Gibbs free energy in relation to emf:

A 
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
Q

Nernst equation:

A 
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
Q

Equation for standard electromotive force:

A

E^ocell = Ered, cathode - Ered, anode

48
Q

What is faraday’s constant and units?

A

10^-5 C/mol*e-

49
Q

Equation for heat released/absorbed in a process:

A 
q = mcdeltaT
q = heat
m = mass
c = specific heat of the substance
deltaT = change in temp
50
Q

What is the ideal gas constant and units?

A

R = 8.3145 J/mol*K

51
Q

Equation for percent yield:

A

% yield = actual yield/theoretical yield x 100%

52
Q

Avogadro’s number and units:

A

6.022 x 10^23 mol^-1

53
Q

Entropy units:

A

J/mol*K

54
Q

1 calorie = ______ J

A

4,184 J

55
Q

Specific heat of water:

A

1 cal/g*K

56
Q

How do Kw, Ka and Kb relate?

A

Kw = Ka * Kb

57
Q

Electrodeposition equation:

A 
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
Q

What is oxidation?

A

loss of electrons

59
Q

What is reduction?

A

gain of electrons

60
Q

What is an oxidizing agent?

A

causes oxidation (loss e-) and becomes reduced itself (gain e-)

61
Q

What is a reducing agent?

A

causes reduction (gain e-) and becomes oxidized itself (loss e-)

62
Q

In electrochemical cells, oxidation happens at the _____.

A

anode

63
Q

In electrochemical cells, reduction happens at the ______.

A

cathode

64
Q

In galvanic cells, the cathode has a _____ reduction potential.

A

more positive

65
Q

In galvanic cells, the anode has a _____ reduction potential.

A

less positive

66
Q

In electrolytic cells, the cathode has a _____ reduction potential.

A

less positive

67
Q

In electrolytic cells, the anode has a _____ reduction potential.

A

more positive

68
Q

If the emf is positive, the cell _____ energy.

A

releases

69
Q

If the emf is negative(?), the cell _____ energy.

A

absorbs

70
Q

Electrons move from _____ to ______ in electrochemical cells.

A

anode to the cathode

71
Q

Current moves from _____ to _____ in electrochemical cells.

A

cathode to anode

72
Q

Definition of an Arrhenius acid

A

dissociate to form an excess of H+ in solution

73
Q

Definition of an Arrhenius base

A

dissociate to form an excess of -OH in solution

74
Q

Definition of a Bronsted-Lowry acid

A

a species that donates H+ ions

75
Q

Definition of a Bronsted-Lowry base

A

a species that accepts H+ ions

76
Q

Definition of a Lewis acid

A

electron pair acceptor

77
Q

Definition of a Lewis base

A

electron pair donor

78
Q

A _____ acid and _____ base will have an equivalence point < 7.

A

strong; weak

79
Q

A _____ acid and _____ base will have an equivalence point = 7.

A

strong;strong

80
Q

A _____ acid and _____ base will have an equivalence point > 7.

A

weak;strong

81
Q

Ammonium is soluble or insoluble in water?

A

soluble

82
Q

Alkali metals soluble or insoluble in water?

A

soluble

83
Q

Nitrate salts soluble or insoluble in water?

A

soluble

84
Q

Acetate salts soluble or insoluble in water?

A

soluble

85
Q

Cl-,Br-, and I- are soluble/insoluble in water with exceptions of ______.

A

soluble; Ag+, Pb2+,Hg22+

86
Q

Sulfate are soluble/insoluble in water with exceptions of ______.

A

soluble; Ca2+, Sr2+, Ba2+, Pb2+

87
Q

Metal oxides are soluble/insoluble in water with exceptions of ______.

A

insoluble; alkali metals, NH4+, CaO, SrO, BaO

88
Q

Hydroxides are soluble/insoluble in water with exceptions of ______.

A

insoluble; alkali metals, NH4+, Ca2+, Sr2+, Ba2+

89
Q

Carbonates are soluble/insoluble in water with exceptions of ______.

A

insoluble; alkali metals, NH4+

90
Q

Phosphates is soluble or insoluble in water?

A

insoluble

91
Q

Sulfides is soluble or insoluble in water?

A

insoluble

92
Q

Sulfites is soluble or insoluble in water?

A

insoluble

93
Q

Equation for how much heat is needed to move from one phase to another and no change in temp:

A 
q = mL
q = heat
m = mass
L = latent heat/enthalpy of an isothermal process (g/cal)
94
Q

Name of a process with constant heat:

A

adiabatic process

95
Q

Name of a process with constant internal energy:

A

isothermal process

96
Q

Name of a process with constant pressure:

A

isobaric process

97
Q

Name of a process with constant volume:

A

isovolumetric/isochoric process

98
Q

What are the standard conditions?

A

298K (25C)
1 atm
1 M conc

99
Q

What is STP?

A

273K (0C)

1 atm

100
Q

What is standard conditions used for?

A

kinetics, equilibrium, thermodynamics

101
Q

What is STP used for?

A

ideal gas calculations

102
Q

Name 8 state functions:

A 
Pressure
Density
Temperature
Volume
Enthalpy
Internal energy
Gibbs free energy
Entropy
103
Q

What is solid to gas phase called?

A

sublimation

104
Q

What is gas to solid phase called?

A

deposition

General Chemistry (8 decks)

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