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# Fire and Ice

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by

## Kerryann Goode

on 30 June 2013

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#### Transcript of Fire and Ice

Heat is a transfer of energy
Phase Changes
Energy is absorbed from surroundings as a material changes from solid to liquid to gas. (COOLING PROCESS).
HEAT
Measured in joules and calories
Fire

and

Ice

by: Kerryann Goode
by: Kerryann Goode
heat
Temperature
- How hot or cold something is.
Convection
- the transfer of heat from one place to another
by the movement of fluids.
- The measurement of the average kinetic energy of molecules in an object or system.
ice
water vapor
water
Change in Temperature:
T
=
+ energy
----------
(mass)(insulated)
T
=
or
Q
MC
------
energy(heat) released
energy(heat) released
energy(heat) absorbed
energy(heat) absorbed
-heat transferred between a solid and a moving fluid when there is temperature difference.
-transferrs from hot to cold
example:
Energy is released to the surroundings as a material changes from gas to liquid to solid (WARMING PROCESS).
Melting
Evaporation
Condensation
Freezing
Due to a temperature difference
Water is a special case:
Most dense at 4 degrees Celsius
Expands as it gets closer to freezing, 4 degrees C to 0 degrees C, and expands from 4 degrees C upward
Less dense in its solid form (ice) than liquid (water)
Gases expand more than liquids
Thermal Expansion
Materials expand when heated.
Is a transfer of energy
Heat is always transferred from hot to cold
Convection:
movement of heated material (fluids)
The air above the fire is heated by convection
Electromagnetic waves
Does not require any physical substance to transfer any energy
It can travel through the vacuum of space
Conduction:
Direct transfer of heat from molecule to molecule
The log is being heated by the direct contact with the heat of the flames.
Temperature
measure of average molecular kinetic energy
Molecular kinetic energy is how much molecules are moving
Thermal Energy
a transfer of energy from a higher temperature to a lower temperature.
thermal energy transfered
thermal energy transfered
thermal equilibrium is reached when the temperatures are equal.
Specific Heat Capacity
Different materials will warm up at different rates because each material has its own specific heat capacity.
A substance with a high heat capacity is a substance that requires a relative large quantity of heat to cause a small temperature change.
(water for example)
refers to the amount of heat required to cause a unit of mass (a gram or a kilogram) to change its temperature by 1 degree Celsius.
liquids expand more than solids
The wood dock will up heat slower than the sand under the same temperature of the sun because it has a higher specific heat capacity (1700 J/kg C)
"My feet feel better!"
The sand will heat up quicker than the wood dock because it has a lower specific heat capacity. (830 J/kg C) "Ouch! Hot!"
Thermal energy is transfered from a higher temperature to a lower temperature until thermal equilibrium is reached.
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