1. Section 7.3—Changes in State What’s happening when a frozen ice pack melts?

2. The energy being put into the system is used for breaking IMF’s, not increasing motion (temperature) Change in State To melt or boil, intermolecular forces must be broken Breaking intermolecular forces requires energy A sample with solid & liquid will not rise above the melting point until all the solid is gone. The same is true for a sample of liquid & gas

3. Melting When going from a solid to a liquid, some of the intermolecular forces are broken The Enthalpy of Fusion (H fus ) is the amount of energy needed to melt 1 gram of a substance  The enthalpy of fusion of water is 80.87 cal/g or 334 J/g All samples of a substance melt at the same temperature, but the more you have the longer it takes to melt (requires more energy). Energy needed to melt Mass of the sample Energy needed to melt 1 g

4. Phase Changes with a Positive Enthalpy The energy added during a this type of a phase change is not being used to increase the temperature of a substance, but instead to break the intermolecular forces between molecules to change the state. Energy is absorbed when bonds are broken. ΔH will be positive State changes  -Melting  -Boiling

5. Example Example: Find the enthalpy of fusion of a substance if it takes 5175 J to melt 10.5 g of the substance.

6. Example H = enthalpy (energy) m = mass of sample H fus = enthalpy of fusion H fus = 493 J/g Example: Find the enthalpy of fusion of a substance if it takes 5175 J to melt 10.5 g of the substance.

7. Vaporization When going from a liquid to a gas, all of the rest of the intermolecular forces are broken The Enthalpy of Vaporization (H vap ) is the amount of energy needed to boil 1 gram of a substance  The H vap of water is 547.2 cal/g or 2287 J/g All samples of a substance boil at the same temperature, but the more you have the longer it takes to boil (requires more energy). Energy needed to boil Mass of the sample Energy needed to boil 1 g

8. Example Example: If the enthalpy of vaporization of water is 547.2 cal/g, how many calories are needed to boil 25.0 g of water?

9. Example H = enthalpy (energy) m = mass of sample H fus = enthalpy of fusion  H = 1.37×10 4 cal Example: If the enthalpy of vaporization of water is 547.2 cal/g, how many calories are needed to boil 25.0 g of water?

10. Solid Liquid Gas Melting Vaporizing or Evaporating Condensing Freezing Increasing molecular motion (temperature) Changes in State go in Both Directions

11. Going the other way The energy needed to melt 1 gram (H fus ) is the same as the energy released when 1 gram freezes.  If it takes 547 J to melt a sample, then 547 J would be released when the sample freezes.  H will = -547 J The energy needed to boil 1 gram (H vap ) is the same as the energy released when 1 gram is condensed.  If it takes 2798 J to boil a sample, then 2798 J will be released when a sample is condensed.  H will = -2798 J

12. Phase Changes with a negative Enthalpy The energy being released by the system during this type of a phase change is not being used to decrease the temperature of a substance, but instead to re-form the intermolecular forces between the molecules to change the state to a more organized structure. When forces are being re-formed, energy is released. ΔH will be negative  Condensing  Freezing

13. Example Example: How much energy is released with 157.5 g of water is condensed? H vap water = 547.2 cal/g

14. Example H = enthalpy (energy) m = mass of sample H fus = enthalpy of fusion  H = - 8.6×10 4 cal Example: How much energy is released with 157.5 g of water is condensed? H vap water = 547.2 cal/g Since we’re condensing, we need to “release” energy…  H will be negative!

15. Heating Curves Melting & Freezing Point Boiling & Condensing Point Heating curves show how the temperature changes as energy is added to the sample

16. Going Up & Down +H+H -H-H Moving up the curve requires energy, while moving down releases energy

17. States of Matter on the Curve Gas Only Energy added increases temp Liquid & gas Energy added breaks remaining IMF’s Liquid Only Energy added increases temp Solid & Liquid Energy added breaks IMF’s Solid Only Energy added increases temp

18. Different Heat Capacities Gas Only Cp = 0.48 cal/g°C Liquid Only Cp = 1.00 cal/g°C Solid Only Cp = 0.51 cal/g°C The solid, liquid and gas states absorb water differently—use the correct Cp!

19. Changing States Liquid & gas H vap = 547.2 cal/g Solid & Liquid H fus = 80.87 cal/g

20. Adding steps together If you want to heat ice at -25°C to water at 75°C, you’d have to first warm the ice to zero before it could melt. Then you’d melt the ice Then you’d warm that water from 0°C to your final 75° You can calculate the enthalpy needed for each step and then add them together

21. Example: How many calories are needed to change 15.0 g of ice at -12.0°C to steam at 137.0°C? Example Useful information: Cp ice = 0.51 cal/g°C Cp water = 1.00 cal/g°C Cp steam = 0.48 cal/g°C H fus = 80.87 cal/g H vap = 547.2 cal/g

22. Example: How many calories are needed to change 15.0 g of ice at -12.0°C to steam at 137.0°C? Example Useful information: Cp ice = 0.51 cal/g°C Cp water = 1.00 cal/g°C Cp steam = 0.48 cal/g°C H fus = 80.87 cal/g H vap = 547.2 cal/g Warm ice from -12.0°C to 0°C Melt ice Warm water from 0°C to 100°C Boil water Warm steam from 100°C to 137°C 91.8 cal 1500 cal 1213 cal 8208 cal 266 cal Total energy = 11279 cal

23. Example: How many needed to change 40.5 g of water at 25°C to steam at 142°C? Let’s Practice Useful information: Cp ice = 0.51 cal/g°C Cp water = 1.00 cal/g°C Cp steam = 0.48 cal/g°C H fus = 80.87 cal/g H vap = 547.2 cal/g

24. Example: How many needed to change 40.5 g of water at 25°C to steam at 142°C? Let’s Practice Useful information: Cp ice = 0.51 cal/g°C Cp water = 1.00 cal/g°C Cp steam = 0.48 cal/g°C H fus = 80.87 cal/g H vap = 547.2 cal/g Warm water from 25°C to 100°C Boil water Warm steam from 100°C to 142°C 3038 cal 22162 cal 816 cal Total energy = 26016 cal