1. How would you sort these?

2. AS Chemistry
Unit 2
Introduction

3. Unit Modules Basic concepts in organic chemistry
Alcohols, halogenoalkanes and analysis.
Energy
Resources
Plus assessed practicals.

4. Unit 2, Module 3, Energy Enthalpy Introduction
AS Chemistry
Unit 2, Module 3, Energy
Enthalpy Introduction

5. Objectives - Enthalpy 2.3.1 Enthalpy Changes
Candidates should be able to:
(a) explain that some chemical reactions are accompanied by enthalpy changes, exothermic (ΔH, negative) or endothermic ΔH, positive);
(d) construct a simple enthalpy profile diagram for a reaction to show the difference in the enthalpy of the reactants compared with that of the products;
(e) explain qualitatively, using enthalpy profile diagrams, the term activation energy;
(f) define and use the terms:
(i) standard conditions,
(ii) enthalpy change of reaction,
(iii) enthalpy change of formation,
(iv) enthalpy change of combustion;

6. Practical
We will do two simple test-tube experiments, in each case we add a solid to a liquid:
Hydrochloric acid plus magnesium ribbon.
Water plus ammonium nitrate
For each case, write a prediction of what will happen.

7. Practical
Practical 1:
Put 5 cm depth of hydrochloric acid in a test tube.
Add a piece of magnesium ribbon.
Write down ALL your observations.
Write an equation for what happened.
Practical 2:
Put 5 cm depth of water in a test tube.
Add a spatula of ammonium nitrate.

8. Definitions NOW write definitions of: Exothermic reaction
Endothermic reaction
Enthalpy

9. Enthalpy Definitions:
Enthalpy, H, is the heat content that is stored in a system.
Chemical system is the reactants and the products
Surroundings is whatever is outside the chemical system.

10. Enthalpy
It is impossible for us to actually measure how much heat energy is in a system.
What can we measure?
We can measure the energy that is given out or absorbed by a chemical system during a chemical change.
We are actually measuring the heat exchange between the chemical system and its surroundings.

11. The law of conservation of energy
The law of conservation of energy states…
…that energy cannot be created or destroyed, only moved from one place to another.
So if a chemical system releases energy, the surroundings must gain exactly the same amount of energy.

12. Conservation of Energy
Heat loss in a chemical system
= heat gain in the surroundings
We see this as a _________ in temperature
Heat gain in a chemical system
= heat loss from the surroundings
n increase
decrease

13. ΔH = Hproducts - Hreactants
Enthalpy Changes
In a chemical reaction, either the products or the reactants will have more energy.
An enthalpy change, ΔH is:
The heat exchange with the surroundings during a reaction, at constant pressure.
The difference between enthalpy of the products and enthalpy of the reactants:
ΔH = Hproducts - Hreactants

14. Activity
Cut out the boxes and stick in place on the diagram to explain exothermic and endothermic reactions.
Don’t stick them down yet.
Place them where you think they go
We will cover more of the topic and continue to look back at this

15. Exothermic & Endothermic
We now need better definitions of exothermic and endothermic reactions.
For each type of reaction:
Is heat lost to or gained from the surroundings?
Which has the smaller enthalpy, reactants or products?
Is ΔH negative or positive?

16. Exothermic Heat is lost to the surroundings?
The enthalpy of the products is smaller than the enthalpy of the reactants.
H products < H reactants
ΔH is negative.

17. Self heating cans use exothermic reactions

18. Endothermic Heat is gained from the surroundings?
The enthalpy of the products is larger than the enthalpy of the reactants.
H products > H reactants
ΔH is positive.

20. Exothermic Reactions
The most exploited exothermic reaction in the world is…
…combustion of fuels
Write an equation for burning methane (natural gas) in oxygen.
Which have more enthalpy, products or reactants?
Is ΔH positive or negative?

21. CH4(g) + 2O2(g)  CO2(g) + 2H2O(l) ΔH = -890kJ.mol-1
Exothermic Reactions
Combustion of Fuels
Burning methane in oxygen:
CH4(g) + 2O2(g)  CO2(g) + 2H2O(l) ΔH = -890kJ.mol-1
The units are kJ.mol-1 so it is the
amount of energy per mole.

22. Exothermic Reactions Respiration
Probably the most important reaction for living things, it gives out energy so is exothermic:
Glucose + Oxygen  Carbon dioxide + Water
C6H12 O6 (aq) + 6O2(g)  6CO2(g) + 6H2O(l) ΔH = -2801kJ.mol-1

23. Endothermic Reactions
Thermal decomposition of limestone
Endothermic reactions require energy input for them to take place.
CaCO3 (s)  CaO(s) + CO2(g) ΔH = +178 kJ.mol-1

24. Endothermic Reactions
Photosynthesis
Probably the most important endothermic reaction for living things, it requires energy:
6CO2(g) + 6H2O(l)  C6H12 O6 (aq) + 6O2(g) ΔH = +2801kJ.mol-1
What type of energy does it take in?

25. Enthalpy Profile Diagram
A simple enthalpy profile diagram shows:
the symbols and enthalpy of products
the symbols and enthalpy of reactants
the enthalpy change
You need to be able to draw them and include all the features.

26. Enthalpy Profile Diagram
A simple enthalpy profile diagram:
Exothermic

27. Enthalpy Profile Diagram
A simple enthalpy profile diagram:
Endothermic

28. Activation Energy Why doesn’t magnesium spontaneously burn in air?
It’s products have less energy than it’s reactants so there is no reason they can’t form?
Yes there is – Activation energy!
We need an input of energy in the first place to break the bonds and allow the reaction to start.

29. Activation Energy
Once the reaction has been started it is giving out energy so the activation energy can continue to be overcome and the reaction is self-sustaining.

30. An endothermic reaction has activation energy too.

31. Now
Check you have all of the enthalpy mind map complete
Then complete questions 1 and 2 on page 189:
Draw an enthalpy profile for the following reactions
1) You are given the data for the following reaction
CO(g) + NO2 (g)  CO2 (g) + NO (g)
ΔH = -226 kJ mol-1 Ea = kJ mol-1
2) You are given the data for the following reaction
H2 (g) + I2 (g)  2HI (g)
ΔH = +53 kJ mol-1 Ea = kJ mol-1
More questions
a) What does enthalpy mean?
b) What decides if a reaction is endothermic or exothermic?

32. Objectives - Enthalpy 2.3.1 Enthalpy Changes
Candidates should be able to:
(a) explain that some chemical reactions are accompanied by enthalpy changes, exothermic (ΔH, negative) or endothermic ΔH, positive);
(d) construct a simple enthalpy profile diagram for a reaction to show the difference in the enthalpy of the reactants compared with that of the products;
(e) explain qualitatively, using enthalpy profile diagrams, the term activation energy;
(f) define and use the terms:
(i) standard conditions,
(ii) enthalpy change of reaction,
(iii) enthalpy change of formation,
(iv) enthalpy change of combustion;