5 kinetics Flashcards

1
Q

what is a successful collision?

A

when particles react

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2
Q

define activation energy

A

the minimum energy needed for a reaction to occur

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3
Q

what must happen for a reaction to occur?

A

particles must have energy that is higher than the activation energy (E>Ea)

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4
Q

why might a reaction occur slowly?

A

small number of particles have E>Ea

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5
Q

why do most collisions not cause a reaction?

A

small number of particles have E>Ea

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6
Q

if a reaction occurs very slowly because only a small number of particles have E>Ea, why will all particles eventually react?

A

molecules gain energy due to collisions

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7
Q

why do some molecules only have a small amount of energy?

A

collisions cause some molecules to lose energy

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8
Q

define rate of reaction

A

the rate of change in concentration per unit of time

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9
Q

what are the units for rate of reaction?

A

mol dm-3 s-1

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10
Q

what are the things that influence rate of reaction?

A
  1. temperature
  2. pressure
  3. concentration
  4. catalyst
  5. surface area
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11
Q

explain why temperature increase causes rate of reaction to increase

A

more particles have E>Ea
increases frequency of successful collisions

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12
Q

explain why concentration increase causes rate of reaction to increase

A

increase in number of particles per unit of volume
increases frequency of successful collisions

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13
Q

explain why pressure increase causes rate of reaction to increase

A

increase in number of particles per unit of volume
increases frequency of successful collisions

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14
Q

explain why adding a catalyst causes rate of reaction to increase

A

catalyst lowers Ea
so more particles have E>Ea
increasing frequency of successful collisions

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15
Q

explain why surface area increase causes rate of reaction to increase

A

increased number of reactant particles available
increasing frequency of successful collisions

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