1. Chapter 6 Thermochemistry Intro Presentation

2. The Nature of Energy
Energy is the capacity to do work or to produce heat through a process
In chemistry we are concerned with the heat transfer that occurs during chemical reactions
Heat/Energy flows from high to low concentration
The energy of the universe is constant (Law of Conservation of Energy)

4. Law of Conservation of Energy
Energy cannot be created or destroyed, only converted from one form to another via reactions and processes
Energy is classified as either kinetic or potential

6. Potential Energy Energy due to position or composition
Potential energy is able to be converted to work when it is being used

7. Kinetic Energy Energy due to the motion of the object
Depends on the mass of the object and its velocity
Energy is able to be converted from one form (potential) to the other (kinetic)
Always remember Temperature is a measurement of the randomness of a particle and is not the same thing as Heat.

9. Two Ways To Transfer Energy
1. Heat– involves the transfer of energy between two objects due to a difference in temperature
Does not refer to a substance that is contained by an object
Moves from high to low

10. Work Force acting over a distance
PE is transferred through work from one object to another
So we have two ways to transfer energy, heat and work

11. Energy is a State Function
A state function/property is one that depends only on the present state of the system
This means it does not depend on the past/future of the object
A change in the function (property) in going from one state to another is independent of the pathway taken between the two states

13. Work and Heat are NOT State Functions
Energy and enthalpy are
Energy changes are independent of the pathway taken because no matter what, the measured value is always the same
Work and heat are dependent on the pathway that we take

14. Chemical Energy
1. System– Part of the universe that we wish to focus our attention on
Example: Products and reactants
2. Surroundings—Everything else in the universe
Example: Container the reaction takes place in
In chemistry we always take the SYSTEMS point of view

15. Exothermic Process
Any reaction that involves the flow of energy/heat out of the system
From system to surroundings
Represented by a negative sign

16. Endothermic Processes
Any reaction that involves the flow of heat/energy in to the system
From surroundings into system
Use a positive sign to indicate that any process is endothermic

17. First Law of Thermodynamics
States that the energy of the universe is constant
Basically this law is the law of conservation of energy
According to this law, the amount of heat lost in any process should equal the amount of heat gained by some object related to the process

19. Internal Energy
Sum of KE and PE equals the internal energy (E) of the system
In the equation, the sign reflects the systems point of view
If the system works on the surroundings w is (-) because work flows out of system
If the surrounding are working on the system w is (+) because energy will flow into the system

20. Colour scheme Text & Lines Background Shadows Title Text Fills Accent
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Followed
Hyperlink
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21. Sample Graph

22. Picture slide
Bullet 1
Bullet 2

23. Process Flow Design Plan Build Test Evaluate Bullet 1 Bullet 2

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25. Examples of default styles
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Hyperlinks like this
Visited hyperlinks like this
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Text box
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