Kinetics I Flashcards

1
Q

what is activation energy?

A

the minimum amount of energy for a reaction to occur

so bonds can break

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2
Q

what needs to happen for a reaction to take place?

A

-particles must collide in right direction
-particles must have a minimum amount of KE

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3
Q

how does concentration affect rate of reaction?

A

more particles of reactant in a given volume=more frequent collisions=higher chance of reacting

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4
Q

how does temperature affect rate of reaction?

A

more KE=more frequent collisions=higher chance of particles reacting

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5
Q

what are the economic benefits of catalysts?

A

-lower temperature=less money spent=less CO2 produced
-makes products more useful by changing its properties

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6
Q

examples of economic benefits in industry?

A

iron catalyst in ammonia production:
-without iron temp would have to be raised loads for reaction to occur quick enough
∴ would be expensive + less iron would be produced as the reaction is reversible

polyethene made with ziegler-natta catalyst:
-more dense+rigid+higher melting point

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7
Q

how does increased temperature affect rate of reaction (maxwell-boltzmann)?

A

more particles will have the least Ea ∴ be able to react (curve moves right)

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8
Q

how does increasing pressure affect rate of reaction?

A

more particles in given volume of gas ∴ more frequent successful collisions

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9
Q

how does increasing SA affect rate of reaction?

A

increases surface exposure at which collisions can happen

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10
Q

how do catalysts increase rate of reaction?

A

lower Ea by finding alternative pathway for bonds to be broken + re-made ∴ more particles will have enough energy to react

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11
Q

what is heterogeneous catalysis?

A

heterogeneous catalysts are in a different physical state to the reactants
-e.g. solid iron catalyst in haber process used for gas

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12
Q

where does the reaction occur in heterogeneous catalysis?

A

on the surface of the heterogeneous catalyst ∴ increasing SA of it increases amount of molecules that can react at the same time ∴ increasing rate of reaction

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13
Q

what is a homogeneous catalyst?

A

-same physical state as reactant
-catalyst + reactant combine to make intermediate species which reacts to form products + reformed catalyst

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14
Q

what is rate of reaction?

A

change in amount of reactants and products per unit of time

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