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H Chemistry > Unit 3 > Flashcards

Unit 3 Flashcards

(109 cards)

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1
Q

why is it important that a reaction doesn’t happen too slow

A

it won’t be economically viable

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2
Q

why is it important that a reaction doesn’t happen too fast

A

an explosion could occur

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3
Q

why must reaction rates be controlled in industrial processes

A
  1. it won’t be economically viable
  2. an explosion could occur
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4
Q

what can collision theory be used to explain

A

the effect of concentration, pressure, surface area, temperature, and collision geometry

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5
Q

what theory can explain the effect of concentration, pressure, surface area, temperature, and collision geometry

A

collision theory

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6
Q

what does a potential energy diagram show

A

the energy pathway of a reaction

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7
Q

what can be used to show the energy pathway of a reaction

A

potential energy diagram

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8
Q

what is temperature a measure of

A

the average kinetic energy of the particles in a substance

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9
Q

what is the average kinetic energy of the particles in a substance

A

temperature

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10
Q

activation energy

A

the minimum kinetic energy required by colliding particles before a reaction may occur

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11
Q

the minimum kinetic energy required by colliding particles before a reaction may occur

A

activation energy

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12
Q

what can energy distribution diagrams be used to explain

A

the effect of changing temperature on the kinetic energy of particles and reaction rate

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13
Q

what can be used to explain the effect of changing temperature on the kinetic energy of particles and reaction rate

A

energy distribution graphs

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14
Q

what two things must happen before a successful reaction occurs

A
  1. reactants must collide with the correct geometry

AND

  1. posses a minimum energy
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15
Q
  1. reactants must collide with the correct geometry

AND

  1. posses a minimum energy
A

what two things must happen before a successful reaction occurs

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16
Q

what is temperature a measure of

A

the average kinetic energy of the particles in a substance

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17
Q

what is the average kinetic energy of the particles in a substance

A

temperature

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18
Q

activation energy

A

the minimum kinetic energy required by colliding particles before a reaction may occur

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19
Q

the minimum kinetic energy required by colliding particles before a reaction may occur

A

activation energy

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20
Q

what does an energy distribution diagram explain

A

why increasing the temperature increases the reaction rate

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21
Q

why increasing the temperature increases the reaction rate

A

what does an energy distribution diagram explain

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22
Q

reaction profiles

A

show the enthalpy change that occurs in a reaction and the activation energy

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23
Q

what shows the enthalpy change that occurs in a reaction and the activation energy

A

reaction profiles

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24
Q

enthalpy change of exothermic reaction

A

negative enthalpy change

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25
enthalpy change of endothermic reaction
positive enthalpy change
26
what reactions have a negative enthalpy change
exothermic
27
what reactions have a positive enthalpy change
endothermic
28
activated complex
high energy, unstable arrangement of atoms. formed at the top of the activation energy barrier
29
high energy, unstable arrangement of atoms. formed at the top of the activation energy barrier
activated complex
30
what is formed at the top of the activation energy barrier
activated complex
31
when is the activated energy formed
formed at the top of the activation energy barrier
32
how do catalysts speed up reactions
by lowering the activation energy
33
how does increasing temp increase the reaction rate
there is more particles that have energy greater than or equal to the activation energy
34
there is more particles that have energy greater than or equal to the activation energy
how does increasing temp increase the reaction rate
35
enthalpy change reaction
delta H = H(products) - H(reactants)
36
how does increasing conc lead to increase in rate
increases the number of collisions
37
how does increasing pressure lead to increase in rate
increases the number of collisions
38
how does decreasing particle size lead to increase in rate
increases the number of collisions
39
how does the use of a catalyst lead to increase in rate
the activation energy decreases
40
what can you add to decrease the activation energy
a catalyst
41
what two things to consider about rates of reaction graphs
1. the gradient/steepness of the graph 2. where the graph ends
42
1. the gradient/steepness of the graph 2. where the graph ends
what two things to consider about rates of reaction graphs
43
what can the gradient of a reaction graph show
the sleeper the slope, the faster the reaction
44
the enthalpy change of a reaction is _____ ___ ___ ______ _______
independant of the route taken
45
Molar volume
Volume per mole
46
Volume per mole
Molar volume
47
Units for molar volume
L mol^-1
48
What is molar volume dependent on
Temperature
49
What two factors are important in industrial chemistry
Percentage yeild Atom economy
50
Actual yeild
Amount obtained
51
Amount obtained
Actual yeild
52
Theoretical yeild
Amount obtained worth full conversion of the limiting reactant
53
Amount obtained worth full conversion of the limiting reactant
Theoretical yeild
54
Environmental considerations for industrial processes
Minimise waste Avoiding the use or production of toxic substances Making proteomic products that can biodegrade
55
Atom economy
Measure of how much of the products are useful
56
High atom economy = ____ waste
Less
57
Factors influencing industrial processes
Availability, sustainability and cost of feedstock Opportunities for recycling Energy requirements Marketability of by-products Product yeild
58
How to ensure a costly reactant is converted into protect
Excess or less expensive reactant is used
59
Raw material
Substance obtained from nature
60
Feedstock
A chemical which is reacted to produce other chemical products. This can be from extraction or chemical synthesis.
61
Chemical equilibrium involves..
2 way reactions
62
Reversible reaction
One they can do both forwards and backwards
63
The final equilibrium position is _____ whether you start work the product or reactant
The same
64
When will the reverse reaction begin
When products form
65
Eventually, the rages of forward and reverse reactions will become ____
Equal
66
Chemical equilibrium
Equal rates of forwards and backward reactions Constant concentration of products and reactant
67
Equal rates of forwards and backward reactions Constant concentration of products and reactant
Chemical equilibrium
68
Dynamic equilibrium
50% reactants and 50% products.
69
When can dynamic equilibrium only be achieved
In a closed system
70
If a reaction mixture contains less than 50% products where does the equilibrium lie
To the left
71
What can affect the position of equilibrium
Concentration Pressure Temperature
72
Increase or decrease in conc on equilibrium
Reaction no longer at equilibrium
73
Increase in reactant conc Decrease in product conc
Equilibrium position shifts to the side of products
74
Equilibrium position shifts to the side of products
Increase in reactant conc Decrease in product conc
75
Increase in product conc Decrease in reactant conc
Equilibrium position shifts to the side of reactants
76
Equilibrium position shifts to the side of reactants
Increase in product conc Decrease in reactant conc
77
What happens if temp is increased on equilibrium
Reaction will move in the direction which will reduce the temperature and cool the reactants down
78
Why does an increase in concentration lead to the equilibrium shifting to the right
Allows the product concentration to increase
79
What way does the reaction move if temperature increases
In the direction in which heat is used up The endothermic direction
80
What causes.. Equilibrium shifts in the direction in which heat is used up The endothermic direction
Increase temperature
81
What does the reaction do if temperature is decreased
Reaction moves in the direction which will increase the temperature and heat the reaction up Moves in the direction that uses heat up (exothermic)
82
Reaction moves in the direction which will increase the temperature and heat the reaction up Moves in the direction that uses heat up (exothermic)
Decrease in temperature
83
Pressure changes will only affect reactions in which…
There of atleast one gas involved There of a volume change going from reactant to products
84
There of atleast one gas involved There of a volume change going from reactant to products
Requirements for pressure affecting a reaction
85
Equilibrium if pressure is increased
Reaction will move in the direction they will lower the pressure In the direction where the total gas volume is lower
86
Reaction will move in the direction they will lower the pressure In the direction where the total gas volume is lower
Equilibrium of pressure increased
87
Equilibrium of pressure decreased
Reaction will move in the direction that will increase the pressure In the direction where the total gas volume is higher
88
Reaction will move in the direction that will increase the pressure In the direction where the total gas volume is higher
Equilibrium of pressure decreased
89
If pressure decreased, equilibrium would move to the side with the _______ number of moles
Highest
90
If pressure increases, equilibrium would move to the side with the _______ number of moles
Lowest
91
What does equilibrium solely depend on
Products and reactants
92
Catalyst affect on equilibrium
Doesn’t change position of equilibrium
93
What type of reaction is combustion always
Exothermic Negative value
94
Enthalpy of combustion
The enthalpy change that occurs when one mole of a substance burns completely in oxygen With all reactants and products being in their standard states
95
The enthalpy change that occurs when one mole of a substance burns completely in oxygen With all reactants and products being in their standard states
Enthalpy of combustion
96
Balanced equation for Enthalpy of combustion
Must show 1 mole of the substance that is being burnt
97
Molar bond Enthalpy
The energy required to break one mole of X-Y bond
98
2 points about making bonds
Energy released Exothermic -^H
99
Energy released Exothermic -^H
Bonds making
100
Bonds breaking
Energy used Endothermic +^H
101
Energy released Exothermic -^H
Making bonds
102
Bond Enthalpy
Energy required to break 1 mole of a particular bond between a pair of atoms in the gaseous state
103
Energy required to break 1 mole of a particular bond between a pair of atoms in the gaseous state
Bond Enthalpy
104
What is chromatography for
To seperate components present in a mixture
105
To seperate components present in a mixture
Chromatography
106
What does chromatography seperate substances based on
Polarity Molecular size
107
Y axis for chromatography
Quantity of substance
108
X axis for chromatograph
Retention time
109

H Chemistry (3 decks)

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