1. Reaction rates course work

2. Reactions occur when particles of reactant collide with enough energy to react.

3. Collision theory

4. Speeding up reactions
Increasing the chance of effective collision, increases the rate (speed) of reaction.
Factors include:
Surface Area
Concentration
Temperature
Catalyst

5. Extra surface for molecules to collide with.
Surface area
Reactions of solids can only take place at the surface of the solid. If we break a solid into smaller pieces we get a larger surface area and a faster reaction.
Molecules collide with the surface of the solid
Extra surface for molecules to collide with.
Smaller particles  larger surface area  more collisions  faster reaction

6. Surface area
If we grind up a solid to a powder we massively increase the surface area.
We therefore massively increase the rate of any reaction
Slow
Very fast

7. Particles in solution can only react with the solids exposed surface

8. Click here to continue

9. Concentration
Reactions in solution involve dissolved particles. The more crowded (concentrated) the solution, the faster the reaction.
Higher concentration  more particles  more collisions  faster reaction

10. Sodium thiosulphate and rate

12. Temperature
Particles need to have a minimum energy to react (activation energy).
Heating the particles gives them energy.
At higher temperatures particles move faster. As a result there are more collisions per second and so a faster reaction occurs.
Higher temperature  faster particles  more collisions  faster reaction

13. Fair Testing Only change one thing - keep everything else the same.
Variables will usually be:
Concentration, volume, mass
(which ever two you are not measuring in the reaction)

14. Catalysts
Speed up a chemical reaction and remain unchanged as they do this. In biology these are called enzymes as they are biological catalysts

15. Reaction rates
Reactions can be followed by measuring changes in concentration, mass and volume of reactants and products.
We can then use these results to make graphs of the results

17. Calculating the Rate of Reaction
The rate of reaction can be calculated by measuring the :
1. Time taken for the reaction
and
2. One other variable (something that changes) e.g.
Volume (cm3)
Mass (g)
Concentration (moles per litre = moll-1)

18. One other variable is measured by a reactant decreasing or a product being formed

19. Rate = Change (in variable)
Time taken

20. Example 1
Use the graph below to calculate the rate of reaction for the first 20 seconds.

21. Example 2
Use the graph below to calculate the rate of reaction between 5.2 and 10.8 seconds.

22. Rate and Time
For some reactions, a colour change will indicate the end of the reaction.
The only measurement carried out during this type of experiment is time. Therefore the rate equation is slightly changed from:
No other variable measured
Rate = Change (in variable)
Time taken
To:
Rate =
Time taken
Units = per second (s-1)

23. Concentration of sodium thiosulphate and the time taken for the cross to disappear

24. By doing a reciprocal graph it allows us to show the relationship between concentration and rate (speed at which reactants are converted to products due to successful collisions) .

25. Reaction Temp (oC) Time (s) 1 40 35 2 60 12 Example 3
Calculate the reaction rates for the experiments below:
Reaction
Temp (oC)
Time (s) 1 40 35 2 60 12
Rate =
Time taken
Rate = 1 35
= s-1
Rate = 1 12
= s-1

26. Calculating Time from Rate Graphs
Example 4
Use the graph below to calculate the time taken for the reaction when a concentration of 0.6 moll-1 is used.

27. We can rearrange the equation to:
Rate = 1
Time
We can rearrange the equation to: 1 = 1
Time =
Rate 12
Time =
0.08
s-1

28. Which of these would speed up the rate at which magnesium reacts with air?
Use a flame to heat the magnesium.
Use larger strips of magnesium.
Add water.
Coat the magnesium in oil.

29. Which of these would speed up the rate at which magnesium dissolves in acid?
Cool the acid.
Cut up the magnesium.
Add water.
Coat the magnesium in oil.

30. Why does breaking up solids increase the rate of reaction?
Makes more solid.
Creates more energy.
Increases surface area.
Increases the concentration.

31. Why does temperature increase the rate of reaction?
Acts as a catalyst.
Increases the concentration.
Increases number of molecules.
Makes collisions more frequent and harder.

32. Which of the following would not speed up a reaction?
Increasing surface area
Increasing concentration of the solution
Increasing the temperature
Diluting the solution