11A.5 Flashcards

1
Q

what is activation energy

A

the minimum energy colliding particles must possess for the reaction to occur

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2
Q

once enough activation energy is there to reach the transition state the particles can

A

the particles can form products and release energy as they do so

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3
Q

where is the transition state in at energy profile diagram

A

it is at the peak of the curve (page 19)

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4
Q

what are the two groups of catalysts

A
  1. homogenous catalysts
  2. heterogeneous catalysts
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5
Q

what is a homogenous catalyst

A

it is a catalyst that is in the same phase as the reactants

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6
Q

why are CFCs bad

A

there are chlorofluoro carbons and they are responsible for the destruction of the ozone layer

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7
Q

what are examples of homogeneous catalysts

A
  1. reaction between chlorine free radicals from CFCs (caused by ultraviolet light) and Oxone layer
  2. peroxydisulfate and either iron 3+ or 2 +
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8
Q

more information about peroxydusulfate and iron

A

page 20

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9
Q

what is a heterogeneous catalyst

A

it is a catalyst that is in the diff state as the reactant

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10
Q

what are Interstitial hydrides

A

hydrogen bonds with transition metals.

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11
Q

what are two examples of heterogeneous catalysts

A
  1. iron for Haber process
  2. vanaduim(v) oxide for the Contact process
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12
Q

how does the iron catalyst speed up the Haber process

A

Iron forms interstitial hydrides with the hydrogen molecule at which the hydrogen atoms re held in place between the metal ions in the lattice the nitrogen molecules are then absorbed into the metal surface nearby where they react with iron and then ammonia is desorbed from the iron

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13
Q

what is adsorption

A

the adhesion of ions, molecules, or atoms to a surface of a solid

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14
Q

what are the three stages in catalysis involving surface absorption (like the Haber process)

A
  1. adsorption: the reactants are adsorbed into the surface of the metal
  2. reaction: the reactant molecules are held in positions that enable them to react together
  3. desorption: the product molecule leaves the surface
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15
Q

what are the two things that can affect the efficiency of a heterogeneous catalyst and why

A
  1. poisoning: some of the catalysts can be filled with impurities that make them useless to use
  2. promoters: some surfaces of the catalysts aren’t effective for the reaction to take place so promoters are used in order to produce active sites where the reaction can take place
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16
Q

what do three-way catalytic converts do

A

they change unburned hydrocarbons into water and carbon dioxide, its also converts carbon, and carbon monoxide into carbon dioxide, and convert oxides of nitrogen into oxygen and nitrogen

17
Q

aluminum oxide catalyst absorbs more

A

water

18
Q

copper and nickel catalyst absorbs more

A

hydrogen

19
Q

what is an autocatalyst

A

when the reactions product act as a catalyst for the reaction

20
Q

what is an example of an autocatalyst reaction

A

the oxidation of ethanedioic acid by potassium manganate (VII) as manganese(II) formed is the catalysts

21
Q

what does the curve of concentration of reactant x time look for an autocatalyst reaction

A

page 21

22
Q

what are other explanations for the shape of the graph of an autocatalyst reaction

A
  1. the reaction is between a solid and a liquid where the liquid needs to penetrate a specific place before the reaction happens
  2. the reaction is extremely exothermic and the heat isn’t being controlled os the heat speeds up the reaction