Particles

Front 1

All matter consists of matter too small to see

(PT)

Back 1

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Front 2

The particles are always moving (as the temperature increases they move faster)

(PT)

Back 2

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Front 3

The particles have mass

(PT)

Back 3

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Front 4

There are spaces between the particles

(PT)

Back 4

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Front 5

Attractive forces hold the particles together

(PT)

Back 5

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Front 6

Collision theory 1?

Back 6

The reactants must collide

Front 7

Collision theory 2?

Back 7

The reactants must collide with enough energy to react

Front 8

Collision theory 3?

Back 8

The reactants must collide with the correct orientation

Front 9

5 factors affecting rate of reaction?

Back 9

Concentration

Temperature

Surface area

Catalysts

Pressure

Front 10

As the concentration increases there a more particles per unit of volume

-> This increases the chance of collisions and reactant rate

->More collisions with enoughactivation energy and correct orientation

Back 10

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Front 11

As the surface area of reactants increases, there are more available sites for collisions between reactants available

Back 11

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Front 12

Decreasing the size of the reactants increases the surface area

e.g. powders have higher surface areas than chips

Back 12

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Front 13

As the surface area increases, the rate of reaction increases

Back 13

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Front 14

As the temperature increases, the rate of proportional reaction increases (directly proportional)

Back 14

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Front 15

As the temperature increases, the particles gain kinetic energy and move faster

Back 15

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Front 16

As the speed of the particles increases, the greater the chance of collisions and chemical reactions

Back 16

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Front 17

Catalysts speed up the rate of reaction without being consumed by the reaction

Back 17

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Front 18

Some catalysts provide a site for particles to correctly orientate and react

Others participate in the reaction and are reformed at the end

Back 18

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Front 19

Catalysts provide a site for particles to correctly orientate and react

Back 19

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Front 20

Catalysts lower the activation energy of the reaction

Back 20

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Front 21

Homogenous catalyst =?

Back 21

same state as reactants

Front 22

Heterogenous catalyst =?

Back 22

different state to reactants

Front 23

Rate of reaction is inversely proportional to 1/time (the longer the reaction time, the slower the rate)

Back 23

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Front 24

Inversely proportional graph:

time vs concentration, dips from high to low

Back 24

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Front 25

directly proportional graph:

1/time vs concentration, a steady rise in the result line

Back 25

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