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Phases of Matter

Phases of Matter. Solid. Liquid. Gas. Quiz. Visualize it!. Heating/cooling curves:. Heat of vaporization potential energy increases kinetic energy remains the same.  Heat of fusion potential energy increases kinetic energy remains the same. Answers to odd questions page 47-48.

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Phases of Matter

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  1. Phases of Matter Solid Liquid Gas Quiz Visualize it!

  2. Heating/cooling curves: Heat of vaporization potential energy increases kinetic energy remains the same  Heat of fusion potential energy increases kinetic energy remains the same Answers to odd questions page 47-48 Sublimation is when a solid goes directly to a gas without passing through the liquid phase.

  3. K = C + 273 C = K - 273 Answers to odd questions page 49

  4. Q = M * C* Change in T

  5. Heat of fusion is the amount of energy needed to melt one gram of ice into water at 0 degrees Celsius 343 J / g

  6. Heat of vaporization is the amount of heat needed to evaporate 1 gram of water at 100 degrees Celsius Hf = 2260 J /g

  7. Ex: 25 grams of water are cooled from 20 oC to 10 oC What is the # of joules of heat energy released? It involves a change in temp so use the formula Q = M x C x (change in T) M = 25 grams; C = 4.18 J/g x oC Change in T = 10 Answer = 1045 J Ex: What are the total # of Joules needed to heat 150g of ice to water at 0 oC. No temp change and ice to water means heat of fusion. Hf = 334 J/g ; Mass = 150 g Answer: 334J x 150 = 50100J Answers to odd questions page 51 - 52 Ex : How many Joules of heat are needed to vaporize 100g of water to vapor at 100 oC. No temp. change and 100 oC. Hv = 2260 J/g ; Mass = 100 g Answer: 2260J x 100 = 22600 J

  8. Kinetic Molecular Theory Postulates of the Kinetic Molecular Theory of Gases • Gases consist of tiny particles (atoms or molecules) • These particles are so small, compared with the distances between • them, that the volume (size) of the individual particles can be assumed • to be negligible (zero). • 3. The particles are in constant random motion, colliding with the walls of • the container.? These collisions with the walls cause the pressure exerted • by the gas. • 4. The particles are assumed not to attract or to repel each other. • 5. The average kinetic energy of the gas particles is directly proportional • to the Kelvin temperature of the gas

  9. Kinetic Theory and the Gas Laws Dorin, Demmin, Gabel, Chemistry The Study of Matter ?, 3rd?Edition, 1990, page 323 (newer book)

  10. A Gas Sample is Compressed Zumdahl, Zumdahl, DeCoste, World of Chemistry?2002, page 429

  11. Boyle’s Law Timberlake, Chemistry 7th?Edition, page 253

  12. P vs. V (Boyle’s Data) Zumdahl, Zumdahl, DeCoste, World of Chemistry?2002, page 404

  13. Boyle’s Law Illustrated Zumdahl, Zumdahl, DeCoste, World of Chemistry?2002, page 404

  14. Charles?s Law Timberlake, Chemistry 7th?Edition, page 259

  15. Plots of V vs. T (Different Gases) Zumdahl, Zumdahl, DeCoste, World of Chemistry?2002, page 407

  16. Ideal vs. Real Gases No gas is ideal. As the temperature of a gas increases and the pressure on the gas decreases the gas acts more ideally. Answers to odd questions page 54 - 56

  17. Gas Mixtures and Dalton’s Law Dalton’s law states that the pressure of the total system is equal to the sum of all the partial pressures.

  18. Heterogeneous Mixtures Filtration is used to separate Heterogeneous solutions. Large particles which are not dissolved in the solution are easily separated using filters.

  19. Separation of Homogeneous mixtures Distillation Chromotography Answers to Odd questions page 59 Separates substances based on boiling points Chromotography

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