1. Energy

2. Energy Energy – the ability to do work or produce heat
Energy exists in two different forms – kinetic energy & potential energy

3. Potential Energy
Potential energy – energy due to composition or position of an object
Potential energy is stored energy that results from the attractions or repulsions of other objects

4. Kinetic Energy Kinetic energy – the energy of motion
Kinetic energy depends on as objects mass & its velocity
Atoms has mass & they are in motion; therefore they will have kinetic energy

5. Energy
A roller coaster at the top of a hill has a great amount of potential energy.
As the rollercoaster begins to speed down the hill, the potential energy is turned into kinetic energy

6. Energy The SI unit for energy is the joule (J) 1 J = 1 Kgm2 / s2
Another unit of energy that you may be more familiar with is the calorie
calorie – amount of energy required to raise 1 g of water 1°C
1 cal = 4.18 J

7. Energy
The calories that you eat are actually kilocalories or Calories (with a big C)
1000 calories = 1 Kilocalorie = 1 Calorie

8. Energy Conversions Convert 15,500 joules into Calories
15500 J x 1 cal x 1 Cal =
4.18 J cal
3.71 Cal

9. Formulas – Kinetic Energy
KE = ½ mv2
KE = kinetic energy (joules)
m = mass (must be in Kg)
V = velocity (must be in m/s)

10. Formulas – Potential Energy
PE = mgh
PE = Potential Energy (J)
m = mass (Kg)
g = gravitational constant = 9.8 m/s2
h = height (m)

11. Formulas - Work
Work (w) – the energy used to move an object against a force
Force (f) – a push or pull on an object
W = mgd = fd = PE
Work and potential energy can be looked at in the same light

12. Work
It is important to understand that if there is no movement, there is no work done
If I push and push on the demonstration table with all of my might. I may get hot and sweaty and feel like I have done a TON of work, but in reality I have done NO work because the table has not moved

13. Examples
A bowler lifts a 5.4 kg bowling ball 1.6m and then drops it to the ground.
How much work was required to raise the ball?
W = mgd
W = (5.4 kg)(9.8 m/s2)(1.6m)
85 Kgm2/s2 = 85 J

14. Examples How much potential energy does that ball have at this height?
85 J

15. Examples
If the bass is dropped and we assume that all of the potential energy is turned into kinetic energy, at what velocity will the bowling ball hit the ground?
KE = PE = 85J
m = 5.4 Kg
V = ?

16. Examples
KE = ½ mv2
85 J = ½ (5.4 Kg) v2
v2 = 31.5
v = 5.6 m/s

17. More examples
What is the kinetic energy of 1 atom of Ar moving at 650 m/s?
KE = ½ mv2
1atom Ar x mol Ar x g Ar x 1 Kg Ar =
6.02 x 1023 atoms mol Ar x 103 g Ar
6.64 x kg Ar

18. More Examples KE = ½ mv2 KE = ½ (6.64 x 10-26)(6502)
KE = 1.4 x J

19. 1st Law of Thermodynamics
1st Law of Thermodynamics – energy is conserved
The law of conservation of energy states that in any chemical reaction or physical process, energy can be converted from one form to another, but it is neither created nor destroyed.

20. 1st Law of Thermodynamics
Since energy can neither be gained nor lost, the change in E can be calculated using:
E = Ef – Ei
In a chemical reaction i indicates reactants and f indicated products

21. E E has 3 parts: A # indicating the magnitude
A sign (+/-) indicating the direction
A unit

22. Thermochemistry
Thermochemistry is the study of heat changes that accompany chemical reactions and phase changes.
In thermochemistry, the system is the specific part of the universe that contains the reaction or process you wish to study.

23. universe = system + surroundings
Thermochemistry
Everything in the universe other than the system is considered the surroundings.
Therefore, the universe is defined as the system plus the surroundings.
universe = system + surroundings

24. Relating E to heat & work
The system can exchange energy with its surroundings in 2 ways: as heat or work
E = q + w
E = change in energy
q = heat
w = work

25. q & w Don’t forget q & w must have signs
In order to get the sign you must look at the system as a box and the surroundings as everything else
System
Surroundings

26. q & w Anything going INTO the box will be +
Anything going OUT of the box will be – + -

27. q & w
If heat is transferred from the surroundings to the system and work is done on the system what are the signs for q & w?
q = +
w = +

28. q & w
If heat is lost to the surroundings and work is done on the system what are the signs for q & w?
q = -
w = +

29. Summary for q & w q + = heat into system q - = heat into surroundings
w + = work done on the system
w - = work done on the surroundings

30. Examples
A system loses 1150 J of heat to the surroundings and does 480 J of work on the surroundings. Calculate E.
E = q + w
E = (-1150J) + (-480J)
E = J

31. Examples
A system absorbs 140 J of heat from the surroundings and does 85 J of work on the surroundings. Calculate E.
E = q + w
E = (+ 140J) + (-85J)
E = + 55 J

32. Endothermic & Exothermic
system absorbs heat
Heat flows into the system
Temperature goes down
Exothermic
Heat flows out of the system and into the surroundings
Temperature goes up
Only look at heat (q) to determine if the system is endo or exo