3b)i) - Collision Theory Flashcards

1
Q

How must reaction rates be controlled

A

Reaction rates must be controlled in industrial processes. If the rate is too low then the process will not be economically viable. If it is too high there will be a risk of explosion

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2
Q

What does collision theory state

A

Collision theory states that before a reaction can take place, the particles must collide with each other

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3
Q

What happens by decreasing particle size

A

By decreasing the particle size of a reactant, we are increasing its surface area

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4
Q

What does a smaller particle size of reactants provide

A

A smaller particle size of reactants provides a greater surface that collisions can take place on

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5
Q

The greater the surface..

A

The greater the surface area the faster the reaction rate

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6
Q

What is the effect of increasing temperature

A

Increasing the temperature, gives the particles more energy, so more particles have the required activation energy

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7
Q

Increasing the temperature..

A

Increasing the temperature increases the reaction rate because the particles collide more often.

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8
Q

What happens if the concentration of reactants is increased

A

If the concentration of reactants is increased, there are more reactant particles moving together

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9
Q

What is the effect of increasing concentration on reaction rate

A

There will be more collisions and so the reaction rate is increased

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10
Q

The higher the concentration of reactants…

A

The higher the concentration of reactants, the faster the reaction rate will be

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11
Q

What happens if the pressure of gaseous reactants is increased

A

If the pressure of gaseous reactants is increased there are more reactant particles for a given volume

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12
Q

What is the effect of pressure of number of collision

A

There will be more collisions and so the reaction rate is increased

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13
Q

The higher the pressure..

A

The higher the pressure of reactants, the faster the rate of a reaction will be

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