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Chemistry 1330H (AKA my death) > Mother Effing Final > Flashcards

Mother Effing Final Flashcards

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1
Q

Reaction Rate is equal to…

A

[A]/time or P=(nRT)/v because n/v= [A]

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2
Q

Factors that Affect Rate (And how)

A

Temp- increased temp= more collisions and KE

Concentration- higher [ ] means more collisions per volume

Physical state- as SA increases, so does rate

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3
Q

Which is constant? Rates or K

A

K

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4
Q

rate of ___1__ = - rate of ___2____

A
  1. Product

2. Reactant

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5
Q

First Order Rate Law and Reaction Order

A

Rate law = K[A]^x where x equals rate order

ln ([Ainitial]/[Afinal])= -Kt

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6
Q

Do First Order Reactions have intermediates?

A

NOPE

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7
Q

Half life equations for first and second order

A

First order half life= 0.693/k

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8
Q

Which is longer? T1/2 of 1st or 2nd order reaction?

A

2nd order

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9
Q

2nd order rate law

A

(1/[A]final)- (1/[A}initial)=Kt

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10
Q

Reaction Mechanisms

A

1) Elementary Steps must be physically reasonable (uni- or bi-molecular)
2) Steps must add to give overall eqn
3) Mechanism must correlate with data and rate determining step

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11
Q

Rate determining Step

A

Slowest step; rate law for this step is the overall rate law

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12
Q

To react, molecules must..?

A

Collide in space and with proper orientation

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13
Q

Activation Energy

A

collisions must have a certain minimum energy (Ea) for a reaction to occur

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14
Q

Arrhenius Equation

A 
K=Ae^(-Ea/RT)
A=frequency factor
Ea= activation Energy
R=ideal gas constant (8.314 J/mol K)
T= temp in Kelvin
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15
Q

Eqn for finding K from different temps

A

ln (k1/k2) = (Ea/RT)((T1-T2)/T1T2)

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16
Q

Catalysts

A

increase reaction rate without being consumed

lowers both forward and reverse Ea by bonding with surface

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17
Q

Homogenous vs heterogenous catalysts

A

homo: in same state (G-G, L-L)
hetero: in different states (G-S)

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18
Q

At equilibrium, do the [products] and [reactants] change?

A

No!

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19
Q

Equilibrium

A

Forward rate = reverse rate

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20
Q

Keq

A

Equilibrium constant

= [products]/[reactants]

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21
Q

What do the coefficients in a reaction do with Keq equation?

A

They become exponents

EX: 3A+B–> 2C so Keq= [C]^2/ ([A]^3[B])

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22
Q

K>1

A

Product Favored

Forward reaction

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23
Q

K

A

Reactant favored

Reverse reaction

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24
Q

Kp =?????

A

= Kc (RT)^(change in n)

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25
Q

When to use Q

A

When you’re not at equilibrium

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26
Q

When Q=K

A

You’re at Equilibrium

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27
Q

When Q

A

reactants need consumed

run reverse reaction

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28
Q

When Q>K

A

products need consumed

run forward reaction

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29
Q

When to use Ice Chart

A

When you have Keq and initial concentrations…. or basically any time you have the initial concentration of anything.

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30
Q

Le chat’s Principle

A

if equilibrium is “disturbed”, a net reaction occurs to reduce the effect of the distrubance; new equilibrium concentrations are established

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31
Q

2SO3 reacts to form 2SO2 + O2. If more O2 is added, what will happen?

A

SO3 will increase while SO2 decreases and O2 increases, then decreases

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32
Q

If you reduce a volume by 1/2, what should you do the the concentrations?

A

Double them!

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33
Q

Nuclear Reactions are ALWAYS what order?

A

First

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34
Q

Are mass changes possible in both chemical and nuclear reactions?

A

No; only nuclear

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35
Q

Atoms can not change identities in (A) chemical or (B) nuclear reactions?

A

chemical

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36
Q

What is traded in a Chemical reaction? In a Nuclear?

A

Chemical- electrons

Nuclear- protons and neutrons

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37
Q

Alpha emission

A

Helium atom

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38
Q

Beta emission

A

-1 on neutron (bottom number)

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39
Q

Positron

A

+1 on neutron (bottom number)

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40
Q

gamma ray

A

positron + electron

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41
Q

change in E= change in m c^2, whats delta m?

A

delta m = (mass/nucleus)(6.02x10^23 nuclei/mol)

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42
Q

U-238 means…?

A

there are 283 nucleons in that atom

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43
Q

nucleon

A

nuetron + proton

Atomic mass

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44
Q

Spontaneous

A

Reaction that occurs under a certain product-favored set o conditions
Delta G1

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45
Q

Exothermic

A

product-favored

delta H1; if T>0, K

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46
Q

Entropy

A

measure of how dispersed the energy is in a system among all the ways energy can be contained

more combinations means higher entropy

State function

47
Q

Boltzmann equation

A

S=k log (W) when S=entropy, K=1.38x10^-23 J/K and W= number of microstates

Large volume means more microstates

48
Q

2nd Law of Thermodynamics

A

any spontaneous process leads to the increasing energy of the universe

delta S of universe >0

49
Q

3rd Law of Thermodyamics

A

Entropy of a perfect crystal at 0 kelvin is 0

50
Q

(increasing/decreasing) temperature means increasing S

A

increasing; more molecular motion

51
Q

Put in increasing order of standard entropy: gas, solid, liquid

A

solid

52
Q

delta S(universe) =?

A 
delta S(sys) + delta S(surr)
NOT equal to 0
53
Q

If delta H(sys)>0, then delta S(surr) is..?

A
54
Q

if delta H(sys)

A

> 0

heat is transferred from system to surroundings

55
Q

delta G(sys) =?

A

delta H(sys)-T delta S(sys)

56
Q

If delta H>0 and delta S

A

> 0(not spontaneous)

57
Q

If delta H0 then delta G is

A
58
Q

If delta H and delta S are >0, then delta G is

A

High temp: 0 (not Spontaneous)

59
Q

If delta H and delta S are

A

High temp:>0 (not spontaneous)

Low temp:

60
Q

Delta G standard can only be used when the [ ] is

A

1M

61
Q

if Q>Keq, then delta G is

A

> 0

net reverse reaction

62
Q

if Q

A
63
Q

If Q=Keq, then delta G is

A

=0

64
Q

Delta G standard =

A

-RT lnKeq

65
Q

delta G=

A

delta G standard+ RT lnQ

66
Q

delta G (increases/decreases) until equilibrium is met

A

decreases

67
Q

Bronsted Acid and base

A

Acid- proton donor

Base- proton acceptor (needs a lone pair)

68
Q

Conjugate pairs

A

chemical species that differ by 1 proton (acid-base pairs)

69
Q

Autoionization of water

A

Water can be an acid or a base

2H2O–> H3O+ + OH-

70
Q

Kw=

A

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

71
Q

when K

A

weak

72
Q

when K»1, the substance is a (strong/weak) electrolyte.

A

Strong

73
Q

HA + H2O reacts to form…

A

H3O+ + A-

74
Q

large Ka vs small Ka

A

Large- strong acid

small- weak acid

75
Q

Ka=

A

([H30+][A-])/[HA]

76
Q

the 6 strong acids

A

HCl, HBr, HI, HNO3, HClO4, H2S04

77
Q

Strong bases

A

alkali hydroxides

78
Q

Ka x Kb=

A

10^-14 or Kw

79
Q

strong acids and bases make (strong/weak) conjugate bases and acids

A

weak

80
Q

Polyprotic acids

A

2+ ionizable protons; harder to remove 2nd proton
more energy so delta G increases
Ka2

81
Q

Across PT Trends on Acid Strength

A

left to right, more acid strength and less proton affinity

Not based on bond strengths

82
Q

Down PT Trends on Acid Strength

A

Going down, acid strength increases and bond strength decreases because smaller atoms mean stronger bonds and waker bonds mean stronger acids

Proton affinity of conjugate bases decreases

83
Q

Oxoacids

A

HmEOn Where m and n are small integers and E is the central Atom

84
Q

Oxoacid strength with PT trends

A

Going down, acid strength decreases as Ka decreases

Adding O increases acid strength because of electron density in OH bond

85
Q

Lewis acid vs base

A

Acid- lone pair acceptor (goes to central atom)

Base- lone pair donor

86
Q

A Bronsted (can/can’t) be a Lewis, but a Lewis (can/can’t) be a Bronsted.

A

Can, can’t

87
Q

Common Ion effect

A

Basically Le Chat’s; When an ion is added to an equilibrium mixture where it’s already present, the equilibrium shifts away from it

88
Q

Henderson- Hasselbach Eqn

A

pH=pKa + log([A-]/[Ha+])

89
Q

From [A-]=[HA+] to [A-]>[HA+], you must add…

A

a strong base

90
Q

From [A-]=[HA+] to [A-]

A

a strong acid

91
Q

A buffer acts to convert a strong acid/base to…

A

a weak acid/base

92
Q

Buffer Capacity

A

how much acid/base can be added before “buffering” is lost

93
Q

Buffer Range

A

How close you are to pKa of your buffer

94
Q

Solubility

A

how much of a solvent dissolves (g/L)

95
Q

If Q=Ksp, the solution is

A

saturated

96
Q

if Q

A

Unsaturated

97
Q

If Q>Ksp, the solution is

A

Super-saturated

98
Q

If something is soluble, delta S must be

A

> 0

99
Q

Redox Reactions

A

transfer electrons from 1 chemical species to another

Conversion of chemical energy to electrical Energy

100
Q

Reducing Agent

A

Is oxidized- positive charge increases

loses electron to substance being reduced

101
Q

Oxidizing agent

A

Is reduced- positive charge decrease

gains electron to substance being oxidized

102
Q

OIL RIG

A

oxidation is loss, reduction is gain (of electrons)

103
Q

Oxidation States

A

sum of oxidation numbers in neutral atom/compound must be zero

104
Q

Good reducing agents:

A

are electropositive (left of PT)
electron rich
low oxidation states

105
Q

Good oxidizing agents:

A

electronegative (right of PT)

high oxidation states

106
Q

Half Reaction Rules

A
  1. assign oxidation numbers
  2. write 1/2 reactions
  3. balance atoms
  4. balance charge
  5. cancel electrons and add

Write 1 eqn for whats oxidized and 1 for whats reduced

107
Q

Standard Reduction Potential

A

at 1 atm, 1 M

E standard >0 means product favored (delta G

108
Q

Galvanic Cells

A

Energy flow from anode (oxidation) to cathode (reduction)

109
Q

When using Hess with Volts, what should you never do to the voltages???

A

MULTIPLY BY THE COEFFICIENT

110
Q

Waterfall analogy

A

Water=electron in an electrochemical cell
Height of waterfall is proportional to the change in voltage between anode and cathode
Volume of water is proportional to the current (number of electrons/second from a to c)

111
Q

-nFE(standard)=

A

delta G standard

112
Q

delta E(standard)=

A

(RT/NF) lnK

113
Q

Nernst Equation

A

E=E(standard) - (0.59 V/n) log Q

Finally nonstandard!!!!

114
Q

Q=

A

[products]/[reactants] = dilute/concentrated

Chemistry 1330H (AKA my death) (1 decks)

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