1. q = ∆HVAPm q = mC∆T q = mC∆T q = mC∆T q=∆HFUSIONm COOLING CURVE
COOLING OF THE GAS SLOPE
q = mC∆T
COOLING OF THE LIQUID SLOPE
q = mC∆T
COOLING OF THE SOLID SLOPE
q = mC∆T
CONDENSATION/VAPORIZATION EQUILIBRIUM PLATEAU.
(G)  (L)
q = ∆HVAPm
FREEZING/MELTING EQUILIBRIUM
PLATEAU. (L)  (S)
q=∆HFUSIONm

2. GAS PHASE
HEATING OF GAS
-No attractions
-Assumes both shape and volume of container,
compressible.
-can be heated infinitely.
EVAPORATION
-Attractions BROKEN as gas heats.
-EVAPORATION occurs at constant temp, POTENTIAL ENERGY CHANGE.
LIQUID PHASE
HEATING OF LIQUID
-”STICKY” attractions
-Assumes shape of container but not the volume,
-Not compressible.
-fluidity, viscosity.
MELTING
-STRONG ATTACTIONS WEAKENED.
-POTENTIAL ENERGY CHANGE.
-energy is gained-endothermic.

3. SOLID GAS PHASE COOLING OF GAS CONDENSATION
-No attractions
-Assumes both shape and volume of container,
compressible.
-can be heated infinitely.
CONDENSATION
-Attractions form as gas cools causing condensation
-Condensations occurs at constant temp, POTENTIAL ENERGY CHANGE.
SOLID
-Strong attractions. lowest energy state.
LIQUID PHASE
COOLING OF LIQUID
-”STICKY” attractions
-Assumes shape of container,
-Not compressible.
-fluidity, viscosity.
FREEZING
-STRONG ATTACTIONS
FORMED
-POTENTIAL ENERGY CHANGE.
-energy is lost-exothermic.

4. COOLING CURVE (a) – first appearance of liquid
(c) – first appearance of solid
(b) – condensation nearly complete
(d) – freezing complete.

5. THE GAS PHASE
No attractions (ideal gas). Real gases do have attractions – proof is they condense.
Move in random straight line motion, collide with each other and container wall.
Assume shape and volume of container.
Compressible – volume is indirect with pressure and direct with temp. Variable density.
At the boiling point, the gas either condenses (cooling curve) or evaporates (heating curve.)
At the higher energy plateau (potential energy) there is an equilibrium of gas and liquid at the same temperature at the same time. And condensation and vaporization ALWAYS occur together.

6. THE LIQUID PHASE
Particles have attractions which are not as strong as in the solid.
Assumes shape but NOT the volume of the container. Not compressible with uniform density.
Particles have some freedom of motion that causes fluidity, however they are not independent as in the gas phase.
Viscosity or “thickness” is a function of attraction strength and temp.
Some of the particles have enough energy to break attractions and escape into the gas phase below the boiling temp. These newly vaporized particles are called VAPOR and exert vapor pressure. The vapor pressure is a direct function of pressure.

7. MELTING/FREEZING EQUILIBRIUM
The solid and liquid exist at equilibrium at the same time at the same temperature (freezing point/melting point).
Melting (fusion) and freezing occur together ALWAYS in an equilibrium. Freezing is faster in a cooling curve, melting is faster in a heating curve.
Attraction strengthen as a substance freezes, attractions weaken as a substance melts.

8. THE SOLID STATE. Assumes neither the shape or volume of its container.
The strongest attractions of any phase.
No momentum, however particles can vibrate in place.
Solids are not compressible and have uniform density.

9. U DO IT NOW!!!
1)CALCULATE THE q WHEN G OF WATER GAS IS COOLED FROM oC to oC.
2)CALCULATE THE HEAT REMOVED WHEN 100 g OF WATER IS CONDENSED AT 100oC.
3)CALCULATE THE HEAT REMOVED WHEN 100g OF WATER LIQUID IS COOLED FROM TO 0.0 oC.
4) CALCULATE THE HEAT REMOVED WHEN 100G OF WATER FREEZES,
5) CALCULATE THE HEAT REMOVED (q) WHEN 100G OF ICE IS COOLED FROM 0.0 C TO -20 C.

10. 1)CALCULATE THE q WHEN 100. 0 G OF WATER GAS IS COOLED FROM 120
1)CALCULATE THE q WHEN G OF WATER GAS IS COOLED FROM oC to oC.
2)CALCULATE THE HEAT REMOVED WHEN 100 g OF WATER IS CONDENSED AT 100oC.
q = mC∆T
Q = 100.0g * J * -20oC =
goC
∆T is negative when T decreases, as is q
q = m-Hvap
Q = 100.0g * J = J g
Condensation is exothermic, has a negative sign. It is the reverse of evaporation.
Condensation is EXOTHERMIC, q is negative

11. 3)CALCULATE THE HEAT REMOVED WHEN 100g OF WATER LIQUID IS COOLED FROM 100.0 TO 0.0 oC.
4) CALCULATE THE HEAT REMOVED WHEN 100G OF WATER FREEZES,
q = mC∆T
q = 100.0g * J * -100oC = J = kJ
goC
q = mHfusion
q = 100.0g * J = J = kJ g

12. Heat of fusion is positive
FREEZING
Q = -
∆Fusion = -
EXOTHERMIC:
Energy EXITS, is released
The heat is equal in number but opposite in sign to heat of fusion
MELTING
Q = +
∆Fusion = +
ENDOTHERMIC
Energy ENTERS, is absorbed
Heat of fusion is positive
CONDENSATION
∆vaporization = -
The heat is equal in number but opposite in sign to heat of vaporization
VAPORIZATION
∆vaporization= +
ENDOTHERMIC:
Heat of vaporization is positive