1. Calculating Energy Changes at Phase Changes

2. The heating rate is 150 J/min.
If the substance takes 4 minutes to melt, how much heat energy was used to melt it?

3. What is the melting point of this substance?
The boiling point?

4. Heat of Fusion
Amount of energy required to change 1 gram of a pure substance from a solid to a liquid at its melting point.
Heat of Fusion = Hf = physical constant.
Hf for water = Joules per gram (Table B)

5. How much heat is absorbed when 10 grams of ice melts at 0oC?
Heat absorbed =
mass of substance X heat of fusion of substance
Q = mHf = (10 g)(333.6 J/g) = 3336 J
Where does that energy go?
Particles must overcome forces of attraction to move farther apart.

7. Heat of Vaporization
Amount of energy required to convert 1 gram of a pure substance from a liquid to a gas at its boiling point.
Heat of vaporization = Hv = physical constant
Hv for water = 2259 J/g

8. How much energy does it take to vaporize 10 g of water?
Q = mHv
Q = (10 g)(2259 J/g) = J
It takes a lot more energy to go from liquid to gas than from solid to liquid. Why?

9. The particles are spreading out a lot more!

10. Heats of fusion & vaporization
Determined in calorimetry experiments.

11. Q = mCgT
Q = mClT
Q = mHv
Q = mCsT
Q =
mHf
Temperature
Time

12. 3 equations for Q Q = mCT Q = mHf Q = mHv
Have to figure out which one to use for a given problem.
Depends which section of heating curve.
Look for hints in the problem.

13. Q = mCT Temperature changed Temperature increased
Temperature decreased
Initial temperature
Start temperature
Final temperature
Ending temperature
From ____ to ____
Water

14. Q = mHf
Ice
Freezing
Melting
At 0C (for H2O)
At constant temperature

15. Q = mHv Steam Boiling Condensation At 100C (for H2O)
At constant temperature

16. Phase Diagrams
A graph of temperature versus pressure that indicates the conditions under which gaseous, liquids, and solid phases of a particular substance exit.
Triple Point – indicates the temperature and pressure conditions at which the solid, liquid, and vapor of the substance can coexist at equilibrium.

17. The critical temperature for carbon dioxide is 31
The critical temperature for carbon dioxide is 31.1°C, and the critical pressure is 73 atm. Above the critical temeprature, the fluid is called super-critical fluid.