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Phase Changes
Phase Change
 It is a transition between solid, liquid, and gaseous
 phases typically involve large amounts of energy
 compared to the specific heat.
Latent Heat
 Is the HEAT released or absorbed by a body during a
 change of state without change of temperature.

               Heat of Fusion
Energy is absorbed from the air to melt solid ice into
liquid water without any change is temperature.
          Heat of Vaporization
Energy is also absorbed to change water into steam
without any change in temperature.
Phase Change
  Diagram   condensation



            evaporation

 Freezing



 Melting
Simple Recall
The change from solid to liquid is.   Melting
The change from liquid to solid.      Freezing
Simple Recall

The change from gas to liquid   Condensation


The change from liquid to gas   Vaporization
Simple Recall
The change from solid to gas.

 Sublimation
The change from gas to solid.

 Deposition
Heat of Phase Change

              Calorimetry
 Nature demands that energy always be conserved:
 The heat lost by objects of decreasing temperature
 must be equal to the heat gained by objects of
 increasing temperature.

 ..Or the state of measurement
 of exchanging quantities of
 heat
Here, if heat is added to a body, then the value is
positive; and if the heat is taken from a body, then the
 value is negative. Since energy (in this case heat) is
                always conserved, then:


     Heat added (+) + Heat taken (-) = 0
               Heat   added = heat taken
Problem Solving

 A glass weighing 30g contains 85g of water at 25o C.
  How much ice at 0 O C will be needed to bring the
  temperature down to 5 O C? The specific heat of glass is
  0.16cal/g, and that of water is 1.00 cal/g.

                                           O           O
 Given : m glass= 30g , m water = 85g at 25 C ,T mix =5 C
 Find : m ice
Problem Solving

 Solution:
      Let H (heat absorbed by ice) ---
            1
            (m )(80cal/g)
                ice
          H 2 (heat absorbed by melted ice) ---
            (m ice )(1.00cal/g .OC )(25 OC – 5O C)
          H 3 (heat given off by glass) ---
            (30 g)(0.16cal/g   . C )(25O C – 5O C)
          H 4 (heat given off by water) ---

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Phase changes

  • 2. Phase Change  It is a transition between solid, liquid, and gaseous phases typically involve large amounts of energy compared to the specific heat.
  • 3. Latent Heat  Is the HEAT released or absorbed by a body during a change of state without change of temperature. Heat of Fusion Energy is absorbed from the air to melt solid ice into liquid water without any change is temperature. Heat of Vaporization Energy is also absorbed to change water into steam without any change in temperature.
  • 4. Phase Change Diagram condensation evaporation Freezing Melting
  • 5. Simple Recall The change from solid to liquid is. Melting The change from liquid to solid. Freezing
  • 6. Simple Recall The change from gas to liquid Condensation The change from liquid to gas Vaporization
  • 7. Simple Recall The change from solid to gas. Sublimation The change from gas to solid. Deposition
  • 8. Heat of Phase Change Calorimetry  Nature demands that energy always be conserved: The heat lost by objects of decreasing temperature must be equal to the heat gained by objects of increasing temperature. ..Or the state of measurement of exchanging quantities of heat
  • 9. Here, if heat is added to a body, then the value is positive; and if the heat is taken from a body, then the value is negative. Since energy (in this case heat) is always conserved, then:  Heat added (+) + Heat taken (-) = 0  Heat added = heat taken
  • 10. Problem Solving  A glass weighing 30g contains 85g of water at 25o C. How much ice at 0 O C will be needed to bring the temperature down to 5 O C? The specific heat of glass is 0.16cal/g, and that of water is 1.00 cal/g. O O  Given : m glass= 30g , m water = 85g at 25 C ,T mix =5 C  Find : m ice
  • 11. Problem Solving  Solution: Let H (heat absorbed by ice) --- 1 (m )(80cal/g) ice H 2 (heat absorbed by melted ice) --- (m ice )(1.00cal/g .OC )(25 OC – 5O C) H 3 (heat given off by glass) --- (30 g)(0.16cal/g . C )(25O C – 5O C) H 4 (heat given off by water) ---