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GCSE AQA Chemistry Flashcards > C8 Rates and Equailibrium > Flashcards

C8 Rates and Equailibrium Flashcards

1
Q

How do you calculate the rate of a reaction using change in amount of reactants?

A

Rate of reaction = change in amount of reactants / time

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2
Q

How do you calculate the rate of a reaction using change in amount of products?

A

Rate of reaction = change in amount of products / time

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3
Q

How do you calculate the rate of a reaction using mass?

A

Rate of reaction = mass / time

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4
Q

How do you calculate the rate of a reaction using volume?

A

Rate of reaction = volume / time

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5
Q

How do you calculate the rate of a reaction using concentration?

A

Rate of reaction = concentration / time

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6
Q

When calculating with mass, why is the initial rate of reaction fast?

A

There are loads of reactant particles to collide with.

  • rate of reaction gradually decreases as the number of reactant particles decrease over time
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7
Q

How does temperature affect the rate of reaction?

A

As temperature increases, particles contain more kinetic energy so there will be more collisions per second.

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8
Q

What is ‘Collision Theory’

A

Chemical reactions can occur ONLY when reacting particles collide with each other in:
- Correct Orientation
- Enough energy

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9
Q

What are factors which affect rate?

A
  • surface area of a solid
  • concentration of a solution
  • pressure of a gas
  • temperature of the reactants
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10
Q

What is activation energy?

A

The minimum amount of energy required for particles to react in a reaction.

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11
Q

Why does the increase surface are to volume ratio increase the rate of reaction?

A

There are more frequent collisions as there is more area for the particles to collide with.

  • the SA:V is directly proportionate to the rate of reaction
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12
Q

Why does the increase in concentration of a solution increase the rate of reaction?

A

There is more of the substance for particles to collide with, meaning that the frequency of collisions increase

  • the concentration is directly proportionate to the rate reaction
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13
Q

Why does the increase in pressure of a gas increase the rate of reaction?

A

The gas particles are more close together, increasing the frequency of succesful collisons.

  • the pressure of gas is directly proportionate to the rate of reaction
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14
Q

Why does higher temperature increase the rate of reaction?

A

An increase in temperature, means that there is an increase in kinetic energy for the particles to collide with.

  • temperature is not directly proportionate to the rate of reaction as there is an increase of energy and increase of frequent collisions
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15
Q

What is a closed system?

A

Apparatus which prevents the escape of reactants and products

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16
Q

What is yield?

A

Amount of product formed

17
Q

What happens when a mixture is at dynamic equalibrium?

A

When the rate of forward reaction equals to rate of the reverse reaction and there is no overall change in the concentrations of reactants and products.

-* this can only occur in a closed system*

18
Q

If equailibrium shifts to the right…..

A

….. amount of yeild (products) increases

19
Q

If equalibrium moves to left….

A

…. amount of reactants increases

20
Q

If you heat up an equalibrium…….

A

….. it will shift towards endothermic direction

21
Q

What are examples of endothermic reactions?

A
  • electrolysis
  • thermal decomposition
  • cracking
  • photosynthesis
22
Q

What are examples of exothermic reactions?

A
  • combustion
  • neutralisation
  • displacement
  • respiration
23
Q

What does anhydrous mean?

A

A substance that dosen’t contain water

24
Q

What is climate change?

A

the change in global weather patterns that could be caused by excess levels of greenhouse gases in the atmosphere

25
Q

What is a hyrdated substance?

A

A substance that contain water in its crystals.

26
Q

What is Le Châtelier’s Principle?

A

when a change in conditions is introduced to a system at equilibrium, the position of equilibrium shifts so as to cancel out the change

GCSE AQA Chemistry Flashcards (15 decks)

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