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Gases -

Gases -. UNIT WRAP-UP Review Practice Stoichiometry Vapor Pressure. Agenda: 4/27. Warm-up: Ideal gas law video Choosing the right gas law formula Practice Problems Gas Stoichiometry You Tube Video Practice problems Dalton’s Law of Partial Pressure States of Matter - Changes

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Gases -

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  1. Gases - UNIT WRAP-UP Review Practice Stoichiometry Vapor Pressure

  2. Agenda: 4/27 • Warm-up: Ideal gas law video • Choosing the right gas law formula • Practice Problems • Gas Stoichiometry • You Tube Video • Practice problems • Dalton’s Law of Partial Pressure • States of Matter - Changes • How do the states of matter change? Why? • Sorting Terms • Read States of Change & write a graphic organizer

  3. Ideal Gas Law: Discovery Ed video

  4. Which formula to use? • Combined Gas Law • Ideal Gas Law

  5. Practice: Ideal & Combined Gas Laws • If four moles of a gas at a pressure of 5.4 atmospheres have a volume of 120 liters, what is the temperature? • If I initially have a gas with a pressure of 84 kPa and a temperature of 35℃ and then I heat it to an additional 230℃, what will be the new pressure? (Assume the volume of the container is constant.)

  6. 3. My car has an internal volume of 2600 liters. If the sun heats the care from a temperature of 20℃ to a temperature of 55℃, what will the pressure inside my car be? (Assume that the initial pressure was 760 mm Hg.) • 4. How many moles of gas (air) are in my car in problem #3?

  7. 5. A toy balloon which is filled with air has an internal pressure of 1.25 atm and a volume of 2.5 L. If I take the balloon to the bottom of the ocean where the pressure is 95 atm, what will be the new volume? • 6. How many moles of gas does the toy balloon hold at 1.25 atm, 2.5 L, and 285 K?

  8. Stoichiometry – with gases • You Tube Video

  9. Gas Stoichiometry • N₂ +3H₂→ 2NH₃ What is the volume of NH₃ at STP if produced if 25.0 g of N₂ is reacted with an excess of H₂? 2KClO₃→ 2KCl + 3O₂ If 5.0 g of KClO₃ is decomposed, what volume of O₂ will be produced at STP? How many grams of KCl are produced in the above problem?

  10. Zn + 2HCl → ZnCl₂ + H₂ • What volume of hydrogen at STP is produced when 2.5 g of zinc react with an excess of hydrochloric acid? • 2AlCl₃→ 2Al + 3Cl₂ • If 10.0 g of aluminum chloride are decomposed, how many molecules of chloride are produced?

  11. Dalton’s Law of Partial Pressures V and T are constant P1 P2 Ptotal= P1 + P2

  12. Dalton’s Law of Partial Pressure Ptotal = P₁+P₂+P₃+Petc. • Mixture of gases (no reaction takes place) • What is the total blood gas pressure for a person having CO₂ partial pressure of 60.1 mm Hg and an O₂ partial pressure of 39.2 mm Hg?

  13. Constant temperature Constant pressure Avogadro’s Law Va number of moles (n) V = constant x n V1/n1 = V2/n2

  14. How are gases related to solids and liquids?

  15. Characteristics of Solids, Liquids & Gases • Sort the terms into 3 columns: S, L, G • (Hint: Look for 3 cards with similar wording and determine which best fits solid, liquid or gas) • Solid Liquid Gas

  16. Read Study Guide pp. 2 - Changes of State • Prepare a graphic organizer to show the changes of state and why they happen • Include terms: solid, liquid, gas, heat, heat energy, melting, boiling, evaporation, forces of attraction, bonds, cool Gases vs. Liquids & Solids

  17. Most substances, like water, can exist in all three states. An iceberg is made of water in solid form. This glass contains liquid water. A cloud is made of water vapor, a type of gas.

  18. How does a substance become a gas? How do solids and liquids differ from gases?

  19. Changing States (Phase changes) Increase Thermal Energy (Heat up) Solid Gas Liquid Decrease Thermal Energy (Cool off)

  20. Melting point Melting - change from solid to liquid Melting point - SPECIFIC temperature when melting occurs. Each pure substance has a SPECIFIC melting point. Examples: M.P. of Water = 0°C (32°F) M.P. of Nitrogen = -209.9 °C (-345.81998 °F) M.P. of Silver = 961.93 °C (1763.474 °F) M.P. of Carbon = 3500.0 °C (6332.0 °F)

  21. Melting Point Particles of a solid vibrate so fast that they break free from their fixed positions. Increasing Thermal Energy Solid Liquid Melting point

  22. Vaporization Vaporization – change from liquid to gas Vaporization happens when particles in a liquid gain enough energy to form a gas. Increasing Thermal Energy Gas Liquid Boiling point

  23. Two Kinds of Vaporization Evaporation – vaporization that takes place only on the surface of the liquid Boiling – when a liquid changes to a gas BELOW its surface as well as above.

  24. Boiling Point Boiling Point – temperature at which a liquid boils Each pure substance has a SPECIFIC boiling point. Examples: B.P. of Water = 100°C (212°F) B.P. of Nitrogen = -195.79 °C (-320.42 °F) B.P. of Silver = 2162 °C (3924 °F) B.P. of Carbon = 4027 °C (7281 °F)

  25. Boiling Point and Melting Point Boiling point Melting point

  26. Standard Curve for all Substances Temperature Thermal Energy Added • As heat decreases, • As heat increases,

  27. Deposition Boiling / Evaporation Sublimation Condensation Freezing Melting WHAT ARE THE CHANGES OF STATE? Which are endothermic? Which are exothermic? GAS SOLID LIQUID

  28. Energy and change of state (phase changes) Energy level Energy change Phase changes MP/BP Entropy= degree of disorder

  29. Vapor Pressure

  30. Vapor pressure • http://www.chem.purdue.edu/gchelp/liquids/vpress.html • Discovery Ed video

  31. Resources for S, L, G • http://www.kentchemistry.com/links/Matter/HeatingCurve.htm

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