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H Chemistry > Unit 3 > Flashcards

Unit 3 Flashcards

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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
Q

enthalpy change of endothermic reaction

A

positive enthalpy change

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26
Q

what reactions have a negative enthalpy change

A

exothermic

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27
Q

what reactions have a positive enthalpy change

A

endothermic

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28
Q

activated complex

A

high energy, unstable arrangement of atoms.

formed at the top of the activation energy barrier

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29
Q

high energy, unstable arrangement of atoms.

formed at the top of the activation energy barrier

A

activated complex

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30
Q

what is formed at the top of the activation energy barrier

A

activated complex

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31
Q

when is the activated energy formed

A

formed at the top of the activation energy barrier

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32
Q

how do catalysts speed up reactions

A

by lowering the activation energy

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33
Q

how does increasing temp increase the reaction rate

A

there is more particles that have energy greater than or equal to the activation energy

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34
Q

there is more particles that have energy greater than or equal to the activation energy

A

how does increasing temp increase the reaction rate

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35
Q

enthalpy change reaction

A

delta H = H(products) - H(reactants)

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36
Q

how does increasing conc lead to increase in rate

A

increases the number of collisions

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37
Q

how does increasing pressure lead to increase in rate

A

increases the number of collisions

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38
Q

how does decreasing particle size lead to increase in rate

A

increases the number of collisions

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39
Q

how does the use of a catalyst lead to increase in rate

A

the activation energy decreases

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40
Q

what can you add to decrease the activation energy

A

a catalyst

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41
Q

what two things to consider about rates of reaction graphs

A
  1. the gradient/steepness of the graph
  2. where the graph ends
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42
Q
  1. the gradient/steepness of the graph
  2. where the graph ends
A

what two things to consider about rates of reaction graphs

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43
Q

what can the gradient of a reaction graph show

A

the sleeper the slope, the faster the reaction

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44
Q

the enthalpy change of a reaction is _____ ___ ___ ______ _______

A

independant of the route taken

45
Q

Molar volume

A

Volume per mole

46
Q

Volume per mole

A

Molar volume

47
Q

Units for molar volume

A

L mol^-1

48
Q

What is molar volume dependent on

A

Temperature

49
Q

What two factors are important in industrial chemistry

A

Percentage yeild

Atom economy

50
Q

Actual yeild

A

Amount obtained

51
Q

Amount obtained

A

Actual yeild

52
Q

Theoretical yeild

A

Amount obtained worth full conversion of the limiting reactant

53
Q

Amount obtained worth full conversion of the limiting reactant

A

Theoretical yeild

54
Q

Environmental considerations for industrial processes

A

Minimise waste

Avoiding the use or production of toxic substances

Making proteomic products that can biodegrade

55
Q

Atom economy

A

Measure of how much of the products are useful

56
Q

High atom economy = ____ waste

A

Less

57
Q

Factors influencing industrial processes

A

Availability, sustainability and cost of feedstock

Opportunities for recycling

Energy requirements

Marketability of by-products

Product yeild

58
Q

How to ensure a costly reactant is converted into protect

A

Excess or less expensive reactant is used

59
Q

Raw material

A

Substance obtained from nature

60
Q

Feedstock

A

A chemical which is reacted to produce other chemical products. This can be from extraction or chemical synthesis.

61
Q

Chemical equilibrium involves..

A

2 way reactions

62
Q

Reversible reaction

A

One they can do both forwards and backwards

63
Q

The final equilibrium position is _____ whether you start work the product or reactant

A

The same

64
Q

When will the reverse reaction begin

A

When products form

65
Q

Eventually, the rages of forward and reverse reactions will become ____

A

Equal

66
Q

Chemical equilibrium

A

Equal rates of forwards and backward reactions

Constant concentration of products and reactant

67
Q

Equal rates of forwards and backward reactions

Constant concentration of products and reactant

A

Chemical equilibrium

68
Q

Dynamic equilibrium

A

50% reactants and 50% products.

69
Q

When can dynamic equilibrium only be achieved

A

In a closed system

70
Q

If a reaction mixture contains less than 50% products where does the equilibrium lie

A

To the left

71
Q

What can affect the position of equilibrium

A

Concentration

Pressure

Temperature

72
Q

Increase or decrease in conc on equilibrium

A

Reaction no longer at equilibrium

73
Q

Increase in reactant conc

Decrease in product conc

A

Equilibrium position shifts to the side of products

74
Q

Equilibrium position shifts to the side of products

A

Increase in reactant conc

Decrease in product conc

75
Q

Increase in product conc

Decrease in reactant conc

A

Equilibrium position shifts to the side of reactants

76
Q

Equilibrium position shifts to the side of reactants

A

Increase in product conc

Decrease in reactant conc

77
Q

What happens if temp is increased on equilibrium

A

Reaction will move in the direction which will reduce the temperature and cool the reactants down

78
Q

Why does an increase in concentration lead to the equilibrium shifting to the right

A

Allows the product concentration to increase

79
Q

What way does the reaction move if temperature increases

A

In the direction in which heat is used up

The endothermic direction

80
Q

What causes..

Equilibrium shifts in the direction in which heat is used up

The endothermic direction

A

Increase temperature

81
Q

What does the reaction do if temperature is decreased

A

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
Q

Reaction moves in the direction which will increase the temperature and heat the reaction up

Moves in the direction that uses heat up (exothermic)

A

Decrease in temperature

83
Q

Pressure changes will only affect reactions in which…

A

There of atleast one gas involved

There of a volume change going from reactant to products

84
Q

There of atleast one gas involved

There of a volume change going from reactant to products

A

Requirements for pressure affecting a reaction

85
Q

Equilibrium if pressure is increased

A

Reaction will move in the direction they will lower the pressure

In the direction where the total gas volume is lower

86
Q

Reaction will move in the direction they will lower the pressure

In the direction where the total gas volume is lower

A

Equilibrium of pressure increased

87
Q

Equilibrium of pressure decreased

A

Reaction will move in the direction that will increase the pressure

In the direction where the total gas volume is higher

88
Q

Reaction will move in the direction that will increase the pressure

In the direction where the total gas volume is higher

A

Equilibrium of pressure decreased

89
Q

If pressure decreased, equilibrium would move to the side with the _______ number of moles

A

Highest

90
Q

If pressure increases, equilibrium would move to the side with the _______ number of moles

A

Lowest

91
Q

What does equilibrium solely depend on

A

Products and reactants

92
Q

Catalyst affect on equilibrium

A

Doesn’t change position of equilibrium

93
Q

What type of reaction is combustion always

A

Exothermic

Negative value

94
Q

Enthalpy of combustion

A

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
Q

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

A

Enthalpy of combustion

96
Q

Balanced equation for Enthalpy of combustion

A

Must show 1 mole of the substance that is being burnt

97
Q

Molar bond Enthalpy

A

The energy required to break one mole of X-Y bond

98
Q

2 points about making bonds

A

Energy released

Exothermic -^H

99
Q

Energy released

Exothermic -^H

A

Bonds making

100
Q

Bonds breaking

A

Energy used

Endothermic +^H

101
Q

Energy released

Exothermic -^H

A

Making bonds

102
Q

Bond Enthalpy

A

Energy required to break 1 mole of a particular bond between a pair of atoms in the gaseous state

103
Q

Energy required to break 1 mole of a particular bond between a pair of atoms in the gaseous state

A

Bond Enthalpy

104
Q

What is chromatography for

A

To seperate components present in a mixture

105
Q

To seperate components present in a mixture

A

Chromatography

106
Q

What does chromatography seperate substances based on

A

Polarity

Molecular size

107
Q

Y axis for chromatography

A

Quantity of substance

108
Q

X axis for chromatograph

A

Retention time

109
Q
A

H Chemistry (3 decks)

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