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Chemistry Paper 2 > Rates Of Reaction > Flashcards

Rates Of Reaction Flashcards

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1
Q

Mean rate of reaction equation

A

Mean rate = quantity product formed / time taken

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2
Q

Definition Of collision theory

A

Chemical reactions can only take place when the reacting particles collide with each other.The collisions must have sufficient energy.

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3
Q

How is the rate of a chemical reaction determined bye

A

The frequency of successful collisions

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4
Q

ROR - increasing particles

A

The more particles the more collisions per second
So the rate of reaction is faster
Increase rate is proportional to concentration

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5
Q

ROR - surface area

A

When we increase the surface area we have more collisions per second so the rate of reaction increases

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6
Q

Purpose of cotton wall

A

To allow carbon dioxide out and prevent acid from splashing out

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7
Q

Definition activation energy

A

The minimum amount of energy the particles must have in order to react

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8
Q

ROR - temperature

A

Increasing the temperature increases the energy of the particles
The particles have more energy to move faster
This increases the frequency of collisions so there is a greater number of collisions per second
More energy more particles can overcome the activation energy barrier and Clyde successfully
Increasing the temperature is proportional to the rate of reaction


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9
Q

Definition catalyst

A

Increase the rate of chemical reactions but are not used up

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10
Q

Why are catalysts good

A

Carry out chemical reactions quickly without increasing the temperature saves money
I’m not you stop that can be reused

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11
Q

Catalysts and activation energy

A

Catalyst provide an alternate pathway for reaction that has a lower activation energy
More particles successfully collide per second

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12
Q

Facts about catalyst x3

A

Do not include catalyst in chemical equations because they’re not used up
Different reactions need different catalysts
Enzymes act as catalysts in organisms

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13
Q

If we heat a reaction is it endothermic or Exothermic

A

Endothermic

Putting energy in

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14
Q

Copper Sulfate is what in the forward direction

A

Endothermic

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15
Q

Closed system

A

No energy can leave or energy

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16
Q

Definition equilibrium

A

When the rate of the forward and backward direction are equal

17
Q

If the system is equilibrium and the changes made to condition then what happens

A

The system responds to counteract the change

18
Q

A = B

What happens if we increase concentration of A

A

More B will form

19
Q

A=B

Decrease concentration of B

A

More A will react to form B

20
Q

A=B

Increase B

A

More B will turn into A

21
Q

If it Exothermic the temperature of the SYSTEM …

A

Increase

22
Q

Of it is endothermic the temperature of the system

A

DECREASES

23
Q

If we increase the temperature the equilibrium shift to the

A

Endothermic

24
Q

What does shift we decrease temperature equilibrium shift

A

Exothermic

25
Q

If we increase the pressure the equilibrium shift to the side with

A

LESS molecules

26
Q

Pressure only effects equilibrium

A

If gases are present

Or same number of particles

27
Q

Explain in terms of particles how and why the rate of reaction changes during the reaction of calcium carbonate with hydrochloric acid (4 marks)

A

Acid particles used up
So concentration decreases
Less frequent collisions per second
So rate of reaction decreases

28
Q

Which is the precipitation

A

The solid

Not aqueous

29
Q

Suggest why catalyst is used in this industrial process

Do not give answers in terms of increasing the rate of reaction

A

Less energy is needed

30
Q

What two pieces of measuring apparatus are needed to find the rate of production of a gas

A

Gas syringe

Stopwatch

31
Q

Rate of reaction minuets or seconds

A

SECONDS

CONVERT

32
Q

Atom economy big numbers

A

YES

33
Q

How will increasing the pressure increase the rate of reaction

A

More collisions per unit time because there are more molecules per unit volume

Chemistry Paper 2 (16 decks)

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