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Science > Rates of Reaction- Chemistry Paper 2 > Flashcards

Rates of Reaction- Chemistry Paper 2 Flashcards

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1
Q

What is the rate of reaction?

A

How quickly the reactants are changed into products

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2
Q

Is the rusting of iron a fast or a slow reaction?

A

Slow

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3
Q

What are the 4 main factors that affect how quickly a reaction goes?

A

Temperature, concentration, surface area, catalysts

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4
Q

What 2 things are collision theory dependent on?

A
  • The frequency of reacting particles, or how often they collide
  • The energy transferred during a collision, as particles have to collide with enough energy to be successful
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5
Q

The more particle collisions…

A

the faster the reaction is

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6
Q

What happens when the temperature is increased?

A

All particles gain more kinetic energy and so move quicker. Collisions will therefore occur more often , resulting in a faster rate of reaction

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7
Q

What does increasing the concentration do?

A

Allow for more frequent collisions and therefore more collisions

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8
Q

What is the concentration?

A

The particles per unit volume

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9
Q

If one of the reactants is a solid, what will breaking it up into smaller pieces do?

A

Increase the surface to volume ratio

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10
Q

Why does increasing the surface area to volume ratio result in more frequent collisions?

A

Because for the same volume particles will have more surface area to work on. This will result in more frequent collisions and so the rate of reaction will be faster.

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11
Q

What does increasing the temperature also increase?

A

The energy of the collisions and the frequency of the collisions

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12
Q

What is activation energy?

A

The minimum energy needed for the particles to react

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13
Q

For a collision to be successful, what must happen?

A

The energy of the particles must be greater than or equal to the activation energy.

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14
Q

What happens if particles don’t have enough energy to react?

A

Then the particles will simply just bounce off each other

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15
Q

What is the rate of a reaction directly proportional to?

A

The frequency of successful collisions

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16
Q

What can decrease the activation energy needed for a reaction to occur?

A

Catalysts

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17
Q

What is the mean rate in reaction equal to?

A

The quantity of reactant used or product formed/time

18
Q

What is a reversible reaction?

A

A reaction where the products can react to become the original reactants

19
Q

What is a dynamic equilibrium?

A

where the rate of the forwards reaction is equal to the rate of the backwards reaction,

20
Q

Dynamic equilibrium must happen in what type of system?

A

A closed system, where none of the reactants or products can leave and nothing else can get in

21
Q

What is Le Chanelier’s principle?

A

The idea that if you change the conditions of a dynamic equilibrium reaction, the system will try to counteract the change.

22
Q

What happens if you raise the temperature of a reaction? (le chantelier’s)

A

The yield of the endothermic reaction will increase and the yield of the exothermic reaction will decrease.

23
Q

What happens if you decrease the temperature of a reaction? le chantelier

A

The yield of the exothermic reaction will increase and the yield of the endothermic reaction will decrease

24
Q

What happens if you increase the pressure of a reaction?(le chantelier)

A

the pressure will favour the side with fewer molecules to try and decrease the pressure

25
Q

What happens if you decrease the pressure of a reaction?

A

the pressure will favour the side with the greatest number of molecules

26
Q

What is the equation for the mean rate of reaction if the quantity of a reactant is measured?

A

mean rate of reaction = quantity of reactant used/ time taken

27
Q

What is the equation for the mean rate of reaction if the quantity of a product is measured?

A

quantity of product formed/ time taken

28
Q

Increasing the pressure…

A

increases the frequency of collisions and hence, increases the rate of reaction

29
Q
A
30
Q

How can the change in a volume be measured?

A

The volume of a gas is measured using a gas syringe, or an upside down burette or measuring cylinder.

31
Q

What is the gradient of a line equal to?

A

The rate of reaction

32
Q

What is an example of a reversible reaction?

A

The production of ammonia

33
Q

What is the Haber process?

A

when nitrogen gas is reacted with hydrogen gas to make ammonia gas. The forward reaction is exothermic.

34
Q

What experiment could be used to see how changes in concentration affect the rates of reaction?

A

1) First, 50 cm^3 of sodium thiosulfate solution should be be measured in a measuring cylinder and then transferred into a flask.
2) With a separate measuring cylinder, 10cm^3 of hydrochloric acid should be measured. The hydrochloric acid should then be added to the flask containing sodium thiosulfate solution and then the stopwatch should be started.
3) A yellow sulphur precipitate forms in the flask
4) The experiment is then repeated with mixtures of sodium thiosulfate solution and water to see how different concentrations affect the time it takes for the cross to disappear

35
Q

What different ways can you measure the formation of products during a reaction?

A
  • Through looking for precipitation
  • Through recording the change in mass
  • By using a gas syringe to measure the volume of gas given off
36
Q

What happens if you heat blue hydrated copper sulfate crystals?

A

The water is driven off and leaves white anhydrous copper sulfate powder. This reaction is endothermic.

37
Q

What happens if you add water to white anhydrous copper sulfate powder?

A

You get the blue copper crystals again and energy is given out - this is exothermic

38
Q

What does anhydrous mean?

A

Without water

39
Q

What is the symbol equation for the thermal decomposition of calcium carbonate?

A

CaCO3 <=> CaO + CO2

40
Q

Is the thermal decomposition of calcium carbonate an endothermic or exothermic reaction?

A

Endothermic, as the calcium carbonate is heated and so takes in heat

41
Q

What happens if you increase the concentration of a reactant?(le chantelier)

A

The system tries to decrease the concentration by making more products

42
Q

What happens if you decrease the concentration of a product?(le chantelier)

A

The system tries to increase the concentration reducing the amount of reactants

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