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Chem 101 Final > Unit 3 > Flashcards

Unit 3 Flashcards

(73 cards)

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1
Q

What is thermodynamics?

A
  • the study of energy and its transformations
  • will the reaction happen
  • interested in starting and ending energies
    concerns entropy and enthalpy
  • can predict if a reaction is favorable or unfavorable le
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2
Q

what is kinetics

A

the study of the processes y which reactants form products
- interested in rates (how fast) and mechanics (how)

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3
Q

what is the first law of thermodynamics

A

energy isn’t created or destroyed it’s converted from one form to another

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4
Q

What is the energy of the universe

A

constant

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5
Q

what’s the change in energy in the universe

A

0

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6
Q

what is the universe made of

A

systems (what you are studying) and surroundings (everything else)

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7
Q

what is the relationship between change in energy of the system and the change in energy of the surroundings

A

energy system= -energy surroundings

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8
Q

what is work

A

force x distance

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9
Q

what is the energy of the system = to

A

heat + work

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10
Q

how do q and w relate to the flow of energy in a system

A

+q= system absorbs heat
- q= system releases heat
+w= system had work done to it by surroundings
-w= system did work to surroundings (lost work energy)

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11
Q

What is enthalpy?

A

the heat of the reaction when the work= 0

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12
Q

what is the energy of the system = when work = 0

A

change in h

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13
Q

What is change in H = to

A

enthalpy

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14
Q

What is standard enthalpy?

A

enthalpy of the reaction when pressure stays at 1.0 atm

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15
Q

what is the relationship between delta h and moles

A

they are proportional

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16
Q

What is an exothermic reaction

A
  • heat energy is released by the system so the surroundings warm
  • enthalpically favorable
  • reactants with weak bonds form products with strong bonds
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17
Q

What is an endothermic reaction?

A

-heat energy is absorbed by the system
-surroundings cool
- reactants with strong bonds form reactants with weak bonds
-enthalpically unfavorable

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18
Q

What is a weak bond

A
  • more reactive and less stable, not a lot of energy is required to break this bond (equivalent to a stretch rubber band)
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19
Q

What is a strong bond

A

less reactive, more stable, more energy required to break

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20
Q

How are strong and weak bonds measured

A

Bond disassociation energy

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21
Q

What is BDE

A

the amount of energy input required to break 1 mole of a bond in the gas phase

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22
Q

How is BDE calculated?

A

add together the bonds that are broken and subtract the ones that are formed

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23
Q

What is entropy

A

the amount of disorder in a system and the amount of ways energy can be distributed in a system

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24
Q

What entropy is favorable

A

the more entropy the more favorable the reaction

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25
What is the relationship between energy placement and entropy
the higher the entropy the more places the energy can be stored
26
When is entropy favorable and unfavorable in a reaction
Entropy is positive and favorable when gas molecules are formed Entropy is negative and unfavorable when you consume gas molecules
27
What is the gibbs free energy formula
delta g= delta h - (t x delta s)
28
What does gibbs free energy tell you
Whether a reaction is spontaneous or not ( will the reaction proceed)
29
When is a reaction spontaneous?
when delta g is negative
30
Does gibbs free energy have anything to do with endothermic and exothermic
no
31
What does - delta h mean?
enthalpically favorable, exothermic
32
What does + delta h mean?
enthalpically unfavorable, endothermic
33
What does - delta s mean?
entropically unfavorable
34
What does + delta s mean?
entropically favorable
35
What does - delta g mean?
spontaneous, favorable
36
What does + delta g mean?
non-spontaneous, unfavorable
37
What is kinetics on an energy coordinate diagram
the dotted line going from reactants to products
38
What is the energy hill
activation energy
39
How does Ea coordinate to reaction time
the larger the Ea the slower the reaction time the smaller the Ea the faster the reaction time
40
What is the transition state?
bonds are 50% broken and 50% formed
41
How does a reaction happen
all atoms are hitting the right spot at the right angle
42
What does kinetic energy show us on an energy coordination diagram?
how fast the reaction will happen
43
How do we determine the reaction rate
k (molarity substance one) (molarity substance two)
44
where do the numbers in front of the substances go in the rate law
they become exponents
45
How can you speed up a reaction?
- increase the temperature - increase molecular concentration - use a catalyst
46
what does a catalyst do
lowers activation energy by bringing molecules closer together
47
Which part of the reaction determines the reaction rate?
the transition state
48
What is equilibrium
where the forward reaction rate= the reverse reaction rate
49
what is the equillibrium expression
- molarities of reverse/ forward - concentration products/ concentration reactants
50
What substances get used during the equilibrium expression and rate laws
-gasses
51
what does keq= 1 mean
equal number of products and reactants
52
what does keq >>1 mean
- has to be greater than 1000 - means the reaction is extensive and goes completely to products
53
what does keq<<1 mean
- smaller than .001 - products are not favored -incomplete reaction, contains mostly reactants
54
what is le chatlier's principle
a system at equilibrium will respond to stress in such a way as to minimize the effect of the stress
55
if you add a reactant the system will:
- turn the reactant into a product - decrease the concentration of reactants - system moves towards products
56
if you remove a product the system will:
-convert reactants to products decrease reactant concentration and increase product concentration -move towards products
57
if you add a product the system will:
-convert products to reactants, -increase the concentration reactants - move towards reactants
58
if you take reactants out the system will:
-turn products into reactants -increase concentration of reactants - shift towards reactants
59
In an exothermic reaction heat is a what
product
60
in an endothermic reaction heat is a what?
reactant
61
What is a bronsted acid
H+ proton donor must have electropositive H atom bound to an electronegative atom
62
What is a Bronsted base
H+ proton acceptor, must have a lone pair that can be used to form a new covalent bond
63
How do you turn a Bronsted acid into a Bronsted base
you remove an H+
64
What is a lewis acid
electron pair acceptor the less electron density, the stronger the Lewis acid
65
What is a lewis base
-Electron pair donator -must have one lone pair it can use to form a new bond - more proton density= stronger lewis base
66
What's the relationship between conjugate bases and acids
the more stable the conjugate base the stronger the parent acid
67
What is Ka
acid dissociation constant
68
what is the Ka formula
concentration products/ concentration reactants doesn't include water
69
what is the relationship between ka and acidity
-the larger the ka the larger the products, the stronger the acid -the smaller the ka the smaller the products, the weaker the acid
69
what is the relationship between ka and acidity
-the larger the ka the larger the products, the stronger the acid -the smaller the ka the smaller the products, the weaker the acid
70
Rank Bronsted acid strength
- strongest acid has the most stable conjugate base, is lower in energy, and unreactive weak base, the larger the ka, the more H3O+ it produces in water, and the more negative the PKA - weakest acid has the least stable conjugate base, the higher in energy reactive strong base, the more positive the PKA, the smaller the Ka
71
what is keq for acids
ka reacting acid/ ka conjugate acid
72
What does CH3 do
strengthens OH bonds making the acids weaker

Chem 101 Final (4 decks)

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