you did work against friction, where did the energy go?
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• You did work against friction, where did the energy go?
Thermal Energy
• Thermal Energy: The total internal Energy
• Internal Energy: The sum of the kinetic and potential energies of the internal motion of particles that make up an object.
What is Heat?• Heat is energy in transfer from an object of
higher temperature to one of lower temperature.
• The quantity of energy transfer from one object to another is because of a difference in temperature.
Cold Hot
Heat Flow
Warm Warm
Change of Phase of State• States of matter
– Solid– Liquid– Gas
• What happens to the temperature when matter is changing states?
Substances in Phase Transfer
40
32
212
40
0
100
FC
Phase Change• Between A-B: The ice is warming to 0oC• Between B-C: Thermal energy melts the ice at 0oC• Between C-D: The water is warm to 100oC• Between D-E: The water boils and changes to vapor at
100oC• After E: The temperature of the vapor increases
Latent Heat
-50
0
50
100
150
Time
Tem
pera
ture
(C
)
A
B
C ED
Thermal Energy Transfer• Conduction:
– Transfer of Kinetic Energy by contact
• Convection:– Heat transfer by the motion of a fluid (e.g. air)
• Radiation:– Electromagnetic waves carry energy
Note: Conduction and Convection require matter
Conduction• Conduction is the transfer of heat through molecular
collisions.• This form of heat transfer best occurs in solids where
molecules are closely packed.• Materials that conduct heat well are called conductors.
(Eg. metals such as copper and iron)
Magnification
Convection• Convection is the transfer of heat though moving fluids.• A fluid is any substance that flows, which includes all
liquids and gases.• Examples include convection ovens and cloud formation.
Convection ?
Radiation (not radioactivity)
• Radiation is the transfer of heat via electromagnetic waves.
• These waves include visible light, but are mostly infrared.
• No matter is required for this type of heat transfer.
• Examples include the sun’s heat and warmth felt from a flame.
Open Space
?Radiation
Heat Transfer Question• Consider a camp fire burning vigorously.
– How is heat normally transferred while warming its viewers?• Radiation
– How is heat transferred when you put a hand in the smoke?• Convection
– How is heat transferred to a stick when it is placed in the hot coals?
• Conduction
• Some situations involve
multiple heat transfer
types like this.
Specific HeatHeat: The energy that flows as a result of a difference in temperature
Q: The symbol for heat. Measured in Joules (J)
C: the symbol for Specific Heat.The amount of energy needed to raise a unit of mass one temperature unit. (J/kg K)
Heat gained
Q: Heat
m: mass
ΔT: Change in Temperature
Q mC T
Sample Heat Problem• How much heat is required to raise the temperature of a
2.4kg gold ingot (c = 129J/kgK) from 23°C to 45°C?
2.4kgQ mc T
2.4 129 22JkgKQ kg C
6811.2Q J
F IT T T 45 23T C C 22T C
Light
Calorimerty
Calorimeter: A device used to measure changes in thermal energy.
Calorimerty depends on the conservation of energy.
Qgained + Qlost = Zero
Calorimerty Example #1A .4kg block of zinc @115°C is placed in .5kg of water @15°C. Find the final temperature.
( ) ( ) 0a a f ai b b f bim c T T m c T T
a a ai b b bif
a a b b
m c T m c TT
m c m c
.4 (388 / )(115 ) .5 (4180 / )(15 )
.4 (388 / ) .5 (4180 / )
o o o o
f o o
kg j kg C C kg j kg C CT
kg J kg C kg J kg C
15.7ofT C
a a a b bm c T m c T
0gained lostQ Q
Heat of fusion Example #1If 5,000J is added to ice at 0oC, how much ice is melted?
Q=mHf Q=mHv
Water Hf=3.34x105J/kg
Water Hv=2.26x106J/kg
/ fm Q H55000 / 3.34 10 /m J x J kg
.015m kgSpecific Heat Phase Change
Calorimerty Example example #2A .1kg block of brass @90°C is placed in .2kg of water @20°C. Find the final temperature.
a a ai b b bif
a a b b
m c T m c TT
m c m c
.1 (376 / )(90 ) .2 (4180 / )(20 )
.1 (376 / ) .2 (4180 / )
o o o o
f o o
kg j kg C C kg j kg C CT
kg J kg C kg J kg C
23.0ofT C
Heat of fusion example #2
How much heat must be transferred to 100g of ice at 00C unit the ice melts and the temperature of the resulting water rises to 200C?
Water Hf=3.34x105J/kg
5
4
.1 (3.34 10 / )
3.34 10
melt ice fQ mH
Q kg x J kg
Q x J
0 0.1 (4180 / )20
8360
heat waterQ mC T
Q kg J kg C C
Q J
43.34 10 8360
41760total
total
Q x J J
Q J
Heat TransferExample 1
A 0.40kg block of iron is heated from 295K to 325K. How much heat is absorbed by the iron?
C=450J/kg K
Q mC T
(.4 )(450 / )(325 295 )Q kg J kg K K K 5400Q J
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