1. Chapter 17 Thermochemistry
Adapted from Stephen L. Cotton

2. Energy Transformations
Thermochemistry- is concerned with heat changes that occur during chemical reactions.
Energy - capacity for doing work or supplying heat.
If within the chemical substances- it is called chemical potential energy
Gasoline contains a significant amount of chemical potential energy

3. Heat is represented by “q”, it is energy that transfers from one object to another, because of a temperature difference between them.
only changes can be detected!
flows from warmer  cooler object

4. Exothermic and Endothermic Processes
Essentially all chemical reactions and changes in physical state involve either:
release of heat, or
absorption of heat

5. In studying heat changes, think of defining these two parts:
the system - the part of the universe on which you focus your attention
the surroundings - includes everything else in the universe

6. Together, the system and it’s surroundings constitute the universe
Thermochemistry is concerned with the flow of heat from the system to it’s surroundings, and vice-versa.

7. Law of Conservation of Energy
-states that in any chemical or physical process, energy is neither created nor destroyed.
All the energy is accounted for as work, stored energy, or heat.
If heat is released by a chemical system then an equal amount will be absorbed by the surroundings.

8. Heat flowing into a system from its surroundings:
defined as positive
q has a positive value
called endothermic
system gains heat (gets warmer) as the surroundings cool down

9. Heat flowing out of a system into its surroundings:
defined as negative
q has a negative value
called exothermic
system loses heat (gets cooler) as the surroundings heat up

10. Fig page 506
On the left, the system (the people) gain heat from its surroundings (the fire)
this is endothermic (q is positive)
On the right, the system (the body) cools as perspiration evaporates, and heat flows to the surroundings
this is exothermic (q is negative)

11. Every reaction has an energy change associated with it
Exothermic reactions release energy, usually in the form of heat.
Endothermic reactions absorb energy
Energy is stored in bonds between atoms

12. Units for Measuring Heat Flow
A calorie is defined as the quantity of heat needed to raise the temperature of 1 g of pure water 1oC.
Used except when referring to food
a Calorie, (written with a capital C), always refers to the energy in food
1 Calorie = 1 kilocalorie = 1000 cal.

13. The calorie is also related to the Joule, the SI unit of heat and energy
named after James Prescott Joule
4.18 J = 1 cal
Heat Capacity - the amount of heat needed to increase the temperature of an object exactly 1 oC
Depends on both the object’s mass and its chemical composition

14. Heat Capacity and Specific Heat
Specific Heat Capacity (abbreviated “c”) - the amount of heat it takes to raise the temperature of 1 gram of the substance by 1oC
often called simply “Specific Heat”
Note Table 17.1, page 508 (next slide)
Water has a HUGE value, when it is compared to other chemicals

15. Table of Specific Heats
Note the tremendous difference in Specific Heat.
Water’s value is VERY HIGH.

16. For water, c = 4. 18 J/(goC) in Joules, and c = 1
For water, c = 4.18 J/(goC) in Joules, and c = 1.00 cal/(goC) in calories.
Thus, for water:
it takes a long time to heat up, and
it takes a long time to cool off!
Water is used as a coolant!
Note Figure 17.4, page 509

17. Specific Heat Units are either: J/(goC) or cal/(g oC)
To calculate, use the formula: q = m x T x C
heat is abbreviated as “q”
m = mass (grams)
T = change in temperature
c = Specific Heat
Units are either: J/(goC) or cal/(g oC)

18. Specific Heat Example G= m=95.4g, T= 48ºC-25ºC=23ºC, q=849J F= c
The temperature of a 95.4 g piece of copper increases from 25ºC to 48ºC when the copper absorbs 849 J of heat. What is the specific heat of copper?
G= m=95.4g, T= 48ºC-25ºC=23ºC, q=849J
F= c
F= q= m x c x T S=

19. Calorimetry
the measurement of the heat into or out of a system for chemical and physical processes.
Based on the fact that the heat released = the heat absorbed.
The device used to measure the absorption or release of heat in chemical or physical processes is called a Calorimeter.

20. Foam cups are excellent heat insulators, and are commonly used as simple calorimeters under constant pressure.
Fig. 17.5, page 511
For systems at constant pressure, the “heat content” is the same as a property called Enthalpy of the system.
(They are good because they are well-insulated.)

21. Two cups are used nestled together for better insulation.
Foam Cup Calorimeter
Two cups are used nestled together for better insulation.

22. Bomb Calorimeter
Calorimetry experiments can be performed at a constant volume using a device called a bomb calorimeter - a closed system.
Used by nutritionists to measure energy content of food.

23. A Bomb Calorimeter

24. Exothermic
The products are lower in energy than the reactants
Thus, energy is released.
ΔH = -395 kJ
The negative sign does not mean negative energy, but instead that energy is lost.

25. C + O2 → CO2 + 395 kJ Energy Reactants Products ® C + O2
395kJ given off
CO2

26. Endothermic
The products are higher in energy than the reactants
Thus, energy is absorbed.
ΔH = +176 kJ
The positive sign means energy is absorbed

27. CaCO3 → CaO + CO2 CaCO3 + 176 kJ → CaO + CO2 Energy Reactants Products
CaO + CO2
176 kJ absorbed
CaCO3

28. Enthalpy
The heat content a substance has at a given temperature and pressure.
Can’t be measured directly because there is no set starting point.
The reactants start with a heat content.
The products end up with a heat content.
So we can measure how much enthalpy changes.

29. Symbol is H.
Change in enthalpy is DH (delta H).
If heat is released, the heat content of the products is lower.
DH is negative. (exothermic)
If heat is absorbed, the heat content of the products is higher.
DH is positive. (endothermic)

30. Thermochemical Equations
To solve these types of problems…you must have
A balanced equation.
Grams of a substance that is in the equation.
∆H produced from the equation.

31. Thermochemical Equation Example
How much heat will be released when 11.8 g of iron reacts with excess O2 according to the following equation?
3Fe + 2O2 → Fe3O4 ∆H = kJ
G= 11.8 g Fe, ∆H= kJ
F= ∆H

32. How do you get the Formula/Solve Step?
F/S=