1. Heat naturally flows from high temperature to low temperature.
Heat as energy
Heat is energy transferred from one object to another because of a difference in temperature
Heat naturally flows from high temperature to low temperature.

2. Heat
Joule determined that a certain amount of mechanical work resulted from a specific amount of heat input. Joule is credited with defining Heat as energy (or transfer of energy)
Heat is measure in calories or Joules.
1cal = 4.186J
1 cal is the amount of heat necessary to raise the temperature of 1 gram of water by 1 degree C.

3. Heat
14-3 Specific Heat
When you heat an object, the temperature rise depends on mass of the object and a property of the material called “specific heat”.
Q = mc(T2-T1)
Q = amount of heat, m = mass, c = specific heat, T = temp.
The higher the heat capacitance, the smaller the temp change for a given amount of heat input.

4. Heat Calorimetry – solving problems
In a closed system, the heat is transferred from the hot object to the cold object or heat lost by one object = heat gained by another.

5. Heat
Latent Heat
When a material changes phases from a solid to liquid or from liquid to gas, a certain amount of energy is involved in the phase change. This is called the latent heat.
Heat of Fusion: heat required to change from a solid to a liquid.
Heat of Vaporization: heat required when changing from liquid to gas.
Q = mL where m = mass and L = latent heat (look this up in a table)
During a phase change, the material’s temperature stays constant.

6. Heat Solving Calorimetry problems Apply conservation of energy
Heat gained = heat lost
If no phase changes occur, each term will have the form Q(gain) = mc(Tf-Ti) or Q(lost) = mc(Ti-Tf)
If phase changes occur, must account for these Q = mL
When the system reaches equilibrium, the final temperature of each substance will have the same value.