1. Adam Jacoway & Craig Drenthe III
Heat
Adam Jacoway
&
Craig Drenthe III

2. Temperature
Temperature- a measure of the average kinetic energy of the substance
Internal Energy- energies associated with atomic motion (proportional to the substance’s temperature)
Thermal Equilibrium- state at which two bodies in physical contact with each other have identical temperature

3. Temperature and Thermal Equilibrium
Thermal Expansion- as temperature of an object increases so does the volume.
Thermal Expansion characteristics of a material are indicated by a quantity called the coefficient of volume expansion.
0˚ C is known as the ice point and melting point
100˚ C is known as steam point or boiling point
0˚ K is known as absolute zero, which is when there is no movement in the molecules.

4. Fahrenheit Celsius Kelvin Temperature Scales
Conversion: TF = 9/5 TC
Celsius
Conversion: T = TC
Kelvin

5. UNITS OF HEAT- joule(J)
Heat- the energy transferred between objects because of a difference in their temperature
UNITS OF HEAT- joule(J)

6. Process
Change of State
Melting
Solid to Liquid
Freezing
Liquid to Solid
Vaporization
Liquid to Gas
Condensation
Gas to Liquid
Sublimation
Solid to Gas
Deposition
Gas to Solid

7. Thermal Conduction
Substances that transfer heat rapidly are known as thermal conductors, while substances that transfer heat slowly are known as thermal insulators.
Convection involves the movement of cold and hot matter, like hot air rising upward over a flame.

8. More definitions
Specific Heat Capacity- the quantity of heat required to raise a unit mass of homogenous material 1K or 1˚C in a specified way given constant pressure and volume
Calorimetry- an experimental procedure used to measure the energy transferred from one substance to another as heat
Phase Change- the physical change of a substance from one state (solid, liquid, or gas) to another at constant temperature and pressure
Latent Heat- the energy per unit mass that is transferred during a phase change of substance

9. Specific Heat Capacity
Q = m•C•ΔT or Cp= Q/m*ΔT
Q= Quantity of Heat (J)
M= Mass (g or kg)
C= Specific Heat (J/g/°C) or (J/kg/K)
T= Temperature (Kelvin or Celsius)

10. Example Problem
What quantity of heat is required to raise the temperature of 450 grams of water from 15°C to 85°C? The specific heat capacity of water is 4.18 J/G/°C

11. Solution
Like any problem in physics, the solution begins by identifying known quantities and relating them to the symbols used in the relevant equation. In this problem, we know the following:
m = 450 g C = 4.18 J/g/°C T initial = 15°C T final = 85°C
We wish to determine the value of Q - the quantity of heat. To do so, we would use the equation Q = m•C•ΔT. The m and the C are known; the ΔT can be determined from the initial and final temperature.
T = Tfinal - Tinitial = 85°C - 15°C = 70.°C
With three of the four quantities of the relevant equation known, we can substitute and solve for Q.
Q = m•C•ΔT = (450 g)•(4.18 J/g/°C)•(70.°C)
Q = J
Q = 1.3x105 J = 130 kJ (rounded to two significant digits)

12. Common Specific Heats

13. A Little More Explanation

14. Some more information