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Latent Heat
PhysicsMontwood High School
R. Casao
Change of StateMatter exists in 3 states:•Solid•Liquid•Gas
water steam
fusion (at melting point)
vaporization (takes place at boiling point)
solidification condensation
Consider water:
at freezing point at boiling point
ice
Heats of Transformation
When energy is absorbed as heat by a solid or liquid, the temperature of the object does not necessarily rise.
The thermal energy may cause the mass to change from one phase, or state, to another.
The amount of energy per unit mass that must be transferred as heat when a mass undergoes a phase change is called the heat of transformation, L.
Heat of Fusion To melt a solid means to change its
from the solid state to the liquid state. This process requires energy because the molecules of the solid must be freed from their rigid structure.
To freeze a liquid to form a solid is the reverse of melting and requires that energy be removed from the liquid so that the molecules can settle into a rigid structure.
Heat of Fusion When the phase change is from
solid to liquid, the sample must absorb heat; when the phase change is from a liquid to solid, the sample must release heat.
The heat of transformation for these phase changes is called the heat of fusion, Lf.
Water: Lf = 334 J/g = 79.5 cal/gfLmQ
Heat of Vaporization To vaporize a liquid means to change it from the
liquid state to the vapor or gas state. This process requires energy because the molecules must be freed from the liquid state.
Condensing a gas to a liquid is the reverse of vaporizing; it requires that energy be removed from the gas so that the molecules can cluster together instead of flying away from each other.
The heat of transformation for these phase changes is called the heat of vaporization, Lv.
Water: Lv = 2256 J/g = 539 cal/gvLmQ
Phase Changes
Copyright 1999, PRENTICE HALL
Chapter 118
Gas-Liquid Equilibration
Copyright 1999, PRENTICE HALL
Chapter 1110
Phase ChangesPhase ChangesEnergy Changes Accompanying Phase Energy Changes Accompanying Phase
ChangesChanges
Copyright 1999, PRENTICE HALL
Chapter 1112
Phase ChangesPhase ChangesHeating CurvesHeating Curves
Copyright 1999, PRENTICE HALL
Chapter 1113
Heating Curve Illustrated
Phase Change Diagram - Water
vaporization
energy in 2260
kJ
fusion
energy in 334 kJ
condensation
energy out
2260 kJ
solidification
energy out 334
kJ
steam(1 kg)
water(1 kg)
ice(1 kg)
Summary: Change of State
Energy involved in heating 1 kg of water
icesteam(ice and water) melting
(334) (420)water
boiling
(water and stream)(2260) energy /
kJ
Summary: from ice to steam
0
100
Heat of Combustion (HC) The amount of heat released per unit
mass or unit volume of a substance when the substance is completely burned.
Heats of combustion are used as a basis for comparing the heating value of fuels, since the fuel that produces the greater amount of heat for a given cost is the more economic.
Equation: CHmQ
Phase Change Example Heat is added to 0.5 kg of water at 20° C.
How many joules of heat energy are required to change the water to steam at 110° C?
Heat has to be added to the water to raise its temperature from 20° C to the boiling point 100° C.
Heat has to be added to vaporize all of the water that is at 100° C.
JQ
CCCkg
JkgTcmQ ooo
167440
2010041865.0
Phase Change Example
Heat has to be added to raise the temperature of all of the steam from 100° C to 110° C.
Total heat energy: Q = 167440 J + 1130000 J + 10050 J = 1307490 J
J1130000QkgJ2260000kg5.0LvmQ
J10050Q
C100C110Ckg
J2010kg5.0TcmQ ooo
Final Temperature Example A 0.3 kg piece of ice at 0° C is placed in 1 kg of
water at 40° C in an insulated container. If no heat is lost to the container, what is the final temperature of the water?
Q lost water = Q gained ice + Q gained ice water (m·c·T)water = m·Lf + (m·c·T)ice water
FFo
oFo
Fo
o
TkgJ1255.8J100200TC
J4186J167440
C0TCkgJ4186kg0.3
kgJ334000kg0.3TC40Ckg
J4186kg1
Final Temperature Example
C.CJ5441.8
JT
TCJ5441.8J
TCJ4186TC
J1255.8J100200J167440
o
o
F
Fo
FoFo
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