1. Thermochemistry
Chapter 17

2. Thermochemistry
Thermochemistry is the study of heat changes that occur during chemical reactions.

3. Energy is the ability to do work or cause change.
Work is force applied over a distance
Potential Energy is stored energy
Kinetic Energy is energy of motion
Chemical Potential Energy is stored within the structural units of chemical substances.

4. Heat Heat (q) is Energy that is transferred from one object to another
Transfer is due to temperature difference between the two substances
Heat ALWAYS travels from hot to cold
Remember, temperature is a measure of the average kinetic energy of a substance

5. Heat CANNOT be detected. the changes CAUSED by heat however can be
ex. Rise in temperature

6. Law of Conservation of Energy
In any chemical or physical process, energy is neither created nor destroyed.
All of the energy involved can be accounted for as Work, Potential Energy, or Heat.

7. Terms for studying heat:
System – what you are focusing on
Surroundings – everything else
Universe = System + Surroundings
Direction of heat flow is always described relative to the system.
Endothermic process – Energy is absorbed by the system from the surroundings (Heats up)
Exothermic process – Energy is released by the system into the surroundings (Cools down)

8. Endothermic vs. Exothermic
Exothermic Lose Heat - q
Endothermic Gain Heat + q

9. Units of Heat
calorie- the quantity of heat needed to raise the temperature of 1 g of pure H2O 1 degree Celsius.
Calorie = 1000 calories = 1 kilocalorie => Dietary Calorie
Joule – the quantity of heat needed to raise the temperature of 1 g of pure H2O, degrees Celsius.
  J = 1 cal

10. Heat Capacity vs. Specific Heat Capacity
Heat capacity – the amount of heat needed to raise the temperature 1 degree Celsius, for any substance
Depends on mass and composition
Specific heat capacity (specific heat) – the amount of heat it takes to raise the temperature of 1 g of a substance 1 degree Celsius.
Depends on composition only

11. Calculation Specific heat = Heat______________
Mass x Change in Temperature
Specific heat (C or Cp)
Heat (q)
Mass (m)
Change in temperature ( ∆T)
q = m C ∆T

12. Measuring and Expressing Heat Changes (change in temperature)
Calorimetry- Accurate and precise measurement of heat change
Instrument – Calorimeter
For systems at constant pressure, the heat content is the same as enthalpy (H)
Heat changes are the same as changes in enthalpy (ΔH)
q = ΔH
Since q = ΔH, then by substitution
ΔH = m x C x ΔT

13. Heat in Changes of State
Molar Heat of Fusion (ΔHfus) – Solid to Liquid
Molar Heat of Vaporization (ΔHvap) – Liquid to Gas
q = ΔH x mass OR q = ΔH x moles
Depends on units of ΔH

14. Phase Change Diagram

15. Phase Changes

16. Group Concept Questions
Your text defines energy as “the ability to do work or to cause change”. Another definition of energy is “the ability to resist a natural tendency”. Explain this definition and provide an example.
A friend of yours reads that the process of water freezing is exothermic. This friend tells you that this can’t be true because exothermic implies “hot”, and ice is cold. Is the process of water freezing exothermic? If so, explain it so your friend can understand it. If not, explain why not.

17. Group Concept Questions
You place hot metal into a beaker of cold water.
Eventually what is true about the temperature of the metal compared to that of the water? Explain why this is true.
 Label this process as endothermic or exothermic if we consider the system to be:
the metal. Explain
the water. Explain

18. Group Concept Questions
The text describes the law of conservation of energy. Is there a law of conservation of heat? Explain why or why not.
What does it mean when the heat for a process is reported with a negative sign?
You place 100.0g of a hot metal in 100.0g of cold water. Which substance (metal or water) undergoes a larger temperature change? Why is this?

19. Group Concept Questions
A desert is very hot during day but quite cold at night. In the Midwest of the United States, the temperature is more constant between day and night in the summer. Why is this?
Explain why aluminum cans make good storage containers for soft drinks.

20. Calorimetry Problems: Changes in Temperature
How much heat is absorbed by 60.0 g of copper when its temperature is raised from 20 oC to 80 oC?
What is the specific heat of a 124 g sample of brass if 3.94 x 103 J raises the temperature of the brass from oC to 97.0 oC?
If 350 J of heat energy are added to 100 g of a metal and the temperature changes by 25 oC, what is the specific heat of the metal? What is the identity of the metal?
10g of an unknown metal requires 39J of energy to increase its temperature from 50 oC to 60 oC. What is the specific heat of the metal? Identify the metal.

21. Calorimetry Problems: Heat Lost = Heat Gained
When 80.0 grams of a certain metal at 90.0 °C was mixed with grams of water at 30.0 °C, the final equilibrium temperature of the mixture was 36.0 °C. What is the specific heat of the metal?
Calculate the specific heat of a metal if a 55.0 g sample of an unknown metal at 99.0 °C causes a 1.7 °C temperature rise when added to g of water at 22.0 °C.

22. Calorimetry Problems: Heat Lost = Heat Gained
A piece of an unknown metal with mass 23.8 g is heated to 100.0ºC and dropped into 50.0 cm3 of water at 24.0ºC. The final temperature of the system is 32.5ºC. What is the specific heat of the metal?
A blacksmith heated an iron bar to 1445ºC. The blacksmith then tempered the metal by dropping it into 42,800 mL of water that had a temperature of 22ºC. The final temperature of the system was 45ºC. What was the mass of the bar? Note: Specific heat of iron is J/g·Cº.

23. Energy and Reactions
How does ENERGY affect REACTIONS

24. Enthalpy
The amount of energy gained or released in a reaction is the ENTHALPY (∆H).
ALL reactions require energy to occur.
The amount of energy needed to occur is called the ACTIVATION ENERGY.
The more energy required for the reaction to occur, the less likely the reaction will happen.
Because of the energy released in exothermic reactions, exothermic reactions are more likely to occur than endothermic reactions.
In other words, they are more spontaneous.

25. Exothermic and Endothermic Reactions

26. Catalysts
Catalysts speed up reactions by lowering the activation energy required for the reaction to occur.
Enzymes are biological catalysts.
Most catalysts work by helping ions and molecules to “line up” the right way so they can react.

27. Reaction Path

28. Entropy
Whether or not a reaction will occur depends on both ENTHALPY and ENTROPY.
Entropy is a measure of disorder.
Increasing disorder is a spontaneous process.
Entropy of States: solid < liquid < gas
Kinetic ..Energy – Gas
Kinetic Energy – Liquid
Kinetic Energy – Solid
Mixing substances, combining or separating elements, and changing the temperature can affect the level of disorder as well.
Mixing gases

29. Spontaneous?
If energy is released and disorder is increased, the reaction will be spontaneous.
In other words, it will happen “on its own.”
If energy is absorbed and disorder decreases, the reaction will be non-spontaneous.
These reactions will need “help” to occur. They can’t do it by themselves.
If one factor is favorable and one is unfavorable, then spontaneity will depend on the values of enthalpy and entropy.