1. and the table of specific heats. and the table of phase changes
THINGS TO REMEMBER
ΔH for temperature changes uses the formula
ΔQ = c m ΔT
and the table of specific heats.
ΔH for phase changes uses the formula
ΔQ = m l
and the table of phase changes

2. STUDY OF THE EFFECTS OF WORK, HEAT AND ENERGY ON A SYSTEM
THERMODYNAMICS
STUDY OF THE EFFECTS OF WORK, HEAT AND ENERGY ON A SYSTEM

3. ZEROTH LAW – Law of Thermodynamic Equilibrium
Heat energy moves from hot to cold objects until a state of thermodynamic equilibrium (same temperature = same KE) exists between the objects

4. FIRST LAW – Law of Conservation of Heat Energy

5. SECOND LAW – Law of Entropy

6. THIRD LAW – Absolute Zero
As the absolute temperature approaches zero (0 K), the entropy of the system approaches zero.

7. Example: An 8.0 g ice cube at -10oC was placed in a Thermos flask containing 100 ml of water at 20oC. The specific heat of ice is 2.05 J/g-K, the specific heat of water is J/g-K and the heat of fusion of ice-water is 334 kJ/g-K. What is the final equilibrium temperature?

8. = 164 J + 2672 J + 33.49 J/oC Tf + 418.6 J/oC Tf – 8372 J
ΔQ = Hgained + Hlost = 0
= cicemice(0 – (-10)oC) + mice (Hf) + cwmice(Tf-0oC ) + cwmw(Tf-20oC)
= (2.05 J/g-oC)(8.0 g)(10oC) + (8.0 g)(334 J/g-oC) J/g-oC)(8.0 g) (Tf) + (4.186 J/g-oC)(100 g)(Tf-20oC)
= 164 J J J/oC Tf J/oC Tf – 8372 J
= J J/oC Tf
Tf = J/(-452 J/oC)
= 12.2 oC