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Chemistry > Kinetics > Flashcards

Kinetics Flashcards

1
Q

What is rate of reaction ?

A

The change of concentration of a reaction( or products) per unit of time.

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2
Q

What is activation energy ?

A

Minimum amount of energy required for particle to collide and for a reaction to begin.

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3
Q

Draw an energy profile graph

A

Notes

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4
Q

What is an exothermix reaction.

A

Reactants more energy than products.

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5
Q

What is an endothermic reaction ?

A

When products have more energy than reactants.

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6
Q

What factors affect rate of reaction ?

A 
Temperature 
Concentration 
Pressure
Surface area 
Catalyst
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7
Q

What is collision theory ?

A

Particles must collide
Particles must have sufficient (activation) energy
Particles must collide with correct orientation.

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8
Q

Why does a reaction not always occur even when particles collide ?

A

There may be insufficient energy or an incorrect orientation.

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9
Q

How does temperature affect rate of reaction and why ??

A

When temperature increases, particles gain more kinetic energy and number of particle collisions per second increases. Higher number of successful collisions. OR new particles have he activation energy so a higher proportion of collisions are successful.

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10
Q

How does concentration affect rate of reaction ??

A

Proportion of successful collisions is the same however there are more particles in the same volume so they collide more frequently and more successful collisions occur.

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11
Q

How does pressure affect rate of reaction ?

A

Same quantity of particles but in smaller volume therefore although the proportion of successful reactions remains the same, the particles collide more frequently. So a higher rate of successful collisions.

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12
Q

How does surface area affect rate of reaction?

A

More particles are able to collide with particles on the other reactant. Therefore there are more total collisions and more likely successful collisions. Proportion of collisions doesn’t change.

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13
Q

How does a catalyst affect rate of reaction ?

A

Decreases activation energy by providing an alternative reaction pathway where less energy is required.

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14
Q

Explain the Maxwell Boltzmann distribution ?

A

In any mixture of moving molecules the speed of particles will vary a great deal; very slow particles with low energy to very fast particles with Hight energy. However, most particles are close to the average speed.

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15
Q

Draw and label a Maxwell Boltzmann distribution.

A

In notes

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16
Q

How can you change kinetic energy of the Maxwell Boltzmann distribution?

A

Increases temperature: activation energy remains the same, most probable and average energy increases. Therefore more particles with activation energy.

Decrease temperature: activation energy remains the same. Most probable and average energy decrease. Fewer particles with activation energy.

17
Q

Draw graphs showing how an increase or decrease in temperature affects a Maxwell boltzmann curve.

A

In notes

18
Q

Draw how adding a catalyst alters a Maxwell Boltzmann distribution.

A

Notes

Lowers activation energy

19
Q

What are the 2 catalyst types ??

A

Heterogenous

Homogenous

20
Q

What is a heterogenous catalyst ??

A

A catalyst in a different phase to (E.g the reactant.

Solid catalyst and liquid reactant)

21
Q

Give an example of what a heterogenous catalyst is used for

A

To convert toxic gases in exhausts to Carbon dioxide and water vapour which are less harmful.

22
Q

What are homogeneous catalysts ?

A

A catalyst in the same phase as the reactant

E.g - both liquids

23
Q

Give an example of what a homogenous catalyst is used for ?

A

Chlorine free radicals depleting the ozone layer

24
Q

What are the advantages of catalysts ?

A

Lowers activation energy therefore making a reaction more economically efficient.
Lowers production costs.
Lowers energy demands meanning less carbon dioxide is produced so less environmental impact.
Not chemically changes so can be reused.

25
Q

Draw a Maxwell Boltzmann curve when half the molecules are removed.

A

On sheet

26
Q

Draw a Maxwell Boltzmann curve when you add a catalyst.

A

On sheet

27
Q

Draw a Maxwell Boltzmann curve when you reduce container volume

A

On sheet

28
Q

Draw a Maxwell Boltzmann curve when you reduce temperature.

A

On sheet

29
Q

Draw a Maxwell Boltzmann curve when add an inert gas.

A

On sheet

30
Q

How can rate of reaction be calculated ?

A

Gas production- has given off during a specific time using gas syringe.
Mass loss- mass lost from reaction(mass will be lost if one of the products is lost as a gas).
Calorimetery- measured amount of light passing through a coloured solution.

31
Q

Suggest one method you could use for removing soluble impurities from a sample of magnesium hydroxide.

A

Wash with cold water.

32
Q

Why is the surface of magnesium rubbish cleaned when investigation its rate of reaction with hydrochloride acid?

A

Otherwise the oxide layer on its surface may affect reactions (MgO).

33
Q

State two differences between magnesium ribbon reacting with water and steam.

A

With water: slow reaction, produced Mg(OH)2

With steam: vigorous and fast reaction, produces MgO

34
Q

How can rate of reaction be calculated ?

A

Gas production- has given off during a specific time using gas syringe.
Mass loss- mass lost from reaction(mass will be lost if one of the products is lost as a gas).
Calorimetery- measured amount of light passing through a coloured solution.

35
Q

Suggest one method you could use for removing soluble impurities from a sample of magnesium hydroxide.

A

Wash with cold water.

36
Q

Why is the surface of magnesium rubbish cleaned when investigation its rate of reaction with hydrochloride acid?

A

Otherwise the oxide layer on its surface may affect reactions (MgO).

37
Q

State two differences between magnesium ribbon reacting with water and steam.

A

With water: slow reaction, produced Mg(OH)2

With steam: vigorous and fast reaction, produces MgO

Chemistry (27 decks)

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