ENERGY:
Et=KE+PE+Q
KE=Kinetic Energy (Motion)
PE=Potential Energy (potential)
Q=Heat (temperature)
Energy is always expressed in terms of Joules (J)
Law of conservation of energy
∆E=oJ
∆E=Ef-Ei=oJ
A System is user defined. It is literally whatever the user wants it to be.
Energy that is added to a system is Endothermic while energy that is released from the system is
Exothermic.
Work is a process that changes the energy of a system.
State Function is the initial condition relative to the final condition.
“∆” = State Function
Temperature is measured in Kelvin (K)
KE=2/3 kT
Measurement of heat energy of a solution
E=mc^2=2/3kT
Study of heat transfers is called:
Thermodynamic
Es=Q+W
(+)= into system
(-)=out system
Heat  calories or joles
Calorie: the amount of energy needed to raise 1ml water’s temperature 1 kelvin
K=C+273
Specific Heat is the energy needed to heat 1 gram of a specific substance 1 degree.
Heat Transfer Equation
Q=mC∆T
Q=heat
m=mass(g)
C=specific heat
∆T=change in temp(K)
Q(-) then heat is released from the system.
Q(+) then heat is added to the system.
Heat always flows high to low.
Questions:
Energy involving motion is called ___________
The amount of energy in the universe is ___________
___________ measures the random motions of components of a substance.
Energy caused by the position of something is called ___________
The ___________ of energy due to a temperature difference is called heat.
Internal Energy is the sum of ___________ and ___________ energies.
Heat is measured in ___________
A ___________ is used to determine the heat associated with a chemical
reaction.
9. The entropy of the universe is always ___________
10. Q=mC(^)T is the ___________formula
11. Q stands for ___________
12. M stands for ___________
13. C stands for ___________
14. (^)T stands for ___________
15. the amount of energy needed to raise 1 ml of water’s temperature 1 degree
kelvin is a ___________
16. Heat is measured in ___________
17. KE stands for ___________
18. PE stands for ___________
19. Energy added to the system is ___________
20. Energy released from the system is ___________
1. Find the specific heat of Water
2. Find the specific heat of Aluminum
3. Find the specific heat of Copper
4. Find the specific heat of Ice
5. Find the specific heat of iron
6. Find the specific heat of Lead
7. Find the specific heat of silver
8. Find the specific heat of steam
9. What is the formula for work?
10. If a piece of metal that is 25 degrees C is placed in a cup of water that is
15 degrees C, what will the temperature of the water be in a few hours
assuming no heat is lost to the environment.
1. If 100 g of water at 90 degrees C is added to 50 g of water at 10
degrees C, estimate the final temperature.
2. A gas absorbs 45 kj of heat and does 20 kj of work. Calculate delta E
3. A gas absorbs 34 kj of heat and does 12 kj of work. Calculate delta E
4. A 35.2 sample of metal X requires 1251 J of energy to heat the sample
by 25 degrees C. Calculate the specific heat capacity of this metal.
5. If it takes 526kj of energy to warm 7.4 g of water by 17 degrees C, how
much energy would be needed to warm 7.4 g of water by 55 degrees
C?