1. 5 week plan
Each week you will have 2 single lessons and 1 double lesson. In those lessons you will learn aspects from Modern Analytical Techniques (MAT) II and Kinetics II. Using the knowledge from Kinetics II you will then plan and carry out an investigation into rates of reaction. The investigation write up will be due in September and is an entrance requirement for Y13. Wk
Single 1
Single 2
Double 1
Kinetics II
Lesson 1
Lesson 2
MAT II 2
Lesson 3
Mini test 3
Rates investigation Intro
Rates investigation trials 4
Test
Rates investigation trials / experiment 5
Rates investigation Experiment
No lessons

2. Kinetics II
Lesson Lesson Lesson Lesson 4 (test)

3. Kinetics II – Lesson 3 Starter… H/W…
If you miss a session you MUST download the PowerPoint from the shared area and collect associated materials, this is your responsibility.
Starter…
Ethanoic acid and ethanol react to form an ester
Write a balanced symbol equation.
What method would you use to measure the rate?
Is the reaction reversible?
H/W…
Revise for your mini assessment next lesson.
Card sort separate
You must complete all homeworks or you will not be allowed onto Y13 chemistry. No excuses

4. What order is the reaction overall?
Hydration of ethyl ethanoate
CH3COOCH2CH3 + H2O ⇌ CH3COOH + CH3CH2OH or
C4H8O2 + H2O ⇌ C2H4O2 + C2H6O
What order is the reaction overall?
What method would we use?

5. Rate equation
Consider the reaction aA + bB  products

6. Rate equation
If we know the initial concentration and the initial rate… we can work out k.

7. r = k[A]1[B]2[C]O 3rd order overall Practice 1
For the reaction A + B + C  D + E, the following data was collected. Determine the order with respect to each of the individual reactants and write the rate equation. Tip… Look for the experiments where only a single reactants concentration had changed and compare that to the rate.
A = As concentration doubles, so does rate therefore 1st order.
B = As concentration doubles, rate quadrupoles therefore 2nd order.
C = As concentration doubles, rate stays the same therefore 0th order.
r = k[A]1[B]2[C]O
3rd order overall

8. r = k[A]1[B]2[C]O Practice 1
For the reaction A + B + C  D + E, the following data was collected. Calculate the value and units for k using experiment 5.
k = r
[A]1[B]2[C]O
k =
[0.1]1[0.5]2[0.1]O
K = 4
k = mol dm-3 s-1
[mol dm-3][mol2 dm-6]
r = k[A]1[B]2[C]O
k = mol-2 dm6 s-1

9. Practice 2
Work out the rate equation for the reaction, between X and Y, using the initial rate data in the table.

10. Order determination
Your task is to determine the overall order of reaction for the forwards and reverse reaction and then write the rate equation for both reactions

11. Order determination C4H8O2 + H2O ⇌ C2H4O2 + C2H6O Forwards
r = k [C4H8O2]2 [H2O]0
Backwards
r = k [C2H4O2]1 [C2H6O]1