1. Ch. 15: Energy and Chemical Change
15.2 Heat

2. Objectives
Describe how a calorimeter is used to measure energy absorbed or released.
Explain the meaning of enthalpy and enthalpy change in chemical reactions and processes.

3. Measuring Heat
Heat changes that occur during chemical and physical processes can be measured accurately and precisely using a calorimeter.
A calorimeter is an insulated device used for measuring the amount of heat absorbed or released during a chemical or physical process.

4. Calorimetry A known mass of water is placed in the insulated chamber.
The amount of energy that this water absorbs or releases can be calculated from the change in temperature that occurs.
A known mass of water is placed in an insulated chamber in the calorimeter to absorb the energy released from the reacting system or to provide the energy absorbed by the system.

5. Example qw = mCwT q = (50.0 g)(4.184 J/g 0C)(6.8 0C) = 1,400 J
sample of lead heated in a beaker, water insulated, lead dropped into water
qw = mCwT
q = (50.0 g)(4.184 J/g 0C)(6.8 0C) = 1,400 J

6. Practice Problems
A sample of metal is heated and put into a calorimeter containing 125 g of water at C. The final temperature of the water is C. How much heat in J is absorbed by the water?
If 335 g of water at C lost 9750 J of heat, what was the final temperature of the water?
The temperature of a sample of water increases from 20 0C to C as it absorbs 5650 J of heat. What is the mass of the sample?

7. Determining Specific Heat
Remember: we calculated the water absorbs 1,400 J. How much energy does the lead release?

8. Determining Specific Heat
The lead releases 1, 420!! qPb = -1,420 J.
If we know the mass of lead (150 g) and the change in temperature of the lead (28.8 0C C = C0), we can calculate the specific heat of lead.
qPb = mCPbT
CPb = q/mT
C = -1,400 J/(150 g)( C)
C = 0.13 J/g 0C

9. Specific Heat Practice Problems
To solve:
Use Q = mwCwΔTw to determine the amount of heat the water absorbs.
This is the same amount of heat the metal releases. (Just change the sign!)
Use the heat, mass of metal (mm), and temperature change of metal (ΔTm) to find the specific heat of the metal (Cm).
Determine the identity of the metal through its specific heat.

10. Chemical Energy and the Universe
Every chemical reaction and change of physical state either releases heat (is exothermic) or absorbs heat (is endothermic).
Endothermic: energy is absorbed
Exothermic: Energy is released

11. Chemical Energy and the Universe
Thermochemistry is the study of heat changes that accompany chemical reactions and phase changes.
The system is the specific part of the universe that contains the reaction or process you wish to study.
Everything else in the universe is considered the surroundings.
The universe = system + surroundings

12. Chemical Energy and the Universe
Consider heat flow in exothermic and endothermic reactions or processes
In summary,
When you break open the heat pack, oxygen from the air enters the pack. The oxygen reacts with iron in the pack in an exothermic reaction described by the following equation.
Energy is a product of the reaction, which means that heat is released.
(EXOTHERMIC)
(ENDOTHERMIC)

13. Enthalpy and Enthalpy Changes
The total amount of energy a substance contains is impossible to measure.
But, for many reactions, the amount of energy lost or gained (CHANGE in energy) can be measured conveniently in a calorimeter.
Reactions in a calorimeter or any lab take place at a constant atmospheric pressure.

14. Enthalpy and Enthalpy Changes
Chemists use the term enthalpy (H) to represent the heat content of a system at constant pressure.
Therefore, the change in enthalpy (H) is the heat absorbed or released in a chemical reaction at constant atmospheric pressure.
Hrxn is the difference between the enthalpy of the substances present at the end of a reaction and the enthalpy of the substances present at the beginning.

15. Enthalpy and Enthalpy Changes
In other words, the difference between the heat contained in the products and the heat contained in the reactants is the enthalpy (heat) of reaction.
Hrxn = Hproducts - Hreactants
In an endothermic reaction, heat is absorbed, which would create a positive enthalpy. In an exothermic reaction, heat is given off, which means the reaction would have a negative enthalpy. Give me an example! Have you ever made ice? Then you have lowered the enthalpy of water! Have you ever melted ice? Then you have raised the enthalpy of water!

16. Note
Recall q was defined as the heat lost or gained in a chemical reaction or process.
If the reaction takes place at constant pressure, q = Hrxn.
(Therefore, Hrxn = mCT)

17. Enthalpy and Enthalpy Changes
4Fe(s) + 3O2(g) Fe2O3(s) kJ
According to the equation, the reaction is exothermic - energy is written as a product.
Therefore, Hreactants has to be greater than Hproduct and Hrxn has to have a negative sign.
The enthalpy change for this reaction can then be indicated by the notation:
Hrxn = kJ
Hot pack equation.
According to the equation, the reactants in this exothermic reaction lose heat, therefore H(rxn) is a negative.
Enthalpy changes for exothermic reactions are always negative.

18. Enthalpy and Enthalpy Changes
Exothermic
Delta H negative

19. Enthalpy and Enthalpy Changes
NH4NO kJ NH4+ (aq) + NO3- (aq)
This reaction is endothermic since energy is a reactant.
Therefore, Hproducts has to be greater than Hreactant and Hrxn has to have a positive sign.
Hrxn = 27 kJ

20. Endothermic Enthalpy Change