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Review + Lesson #8

Review + Lesson #8. Please look at the updated schedule for May on the website!! Wed: 9 +10 Mon: VICTORIA DAY = NO CLASS Wed: Lesson 11 + Review Monday, May 30 th = TEST. Review from Lessons 5 & 6.

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Review + Lesson #8

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  1. Review + Lesson #8 Please look at the updated schedule for May on the website!! Wed: 9 +10 Mon: VICTORIA DAY = NO CLASS Wed: Lesson 11 + Review Monday, May 30th = TEST

  2. Review from Lessons 5 & 6 • How many molecules of hydrogen sulfide will react with 15 molecules of oxygen gas according to the following equation: • 2H2S + 3O22H2O + 2SO2

  3. Review from Lessons 5 & 6 • If 6.0mol of CO2 are produced, how many moles of O2 reacted, according to the following equation: • C2H4 + 3O2 2CO2 + 2H2O

  4. Review from Lessons 5 & 6 • When lithium reacts with water to produce lithium hydroxide and hydrogen gas, how many moles of lithium hydroxide are produced from 2.12 mol lithium?

  5. Review from Lessons 5 & 6 • Solid iron combines with oxygen gas to produce rust (iron (III) oxide. What mass of rust can be formed from a piece of iron with a mass of 10.5g?

  6. Review from Lessons 5 & 6 • When potassium chlorate decomposes to form solid potassium chloride and oxygen gas, how much potassium chlorate is required to produce 156g potassium chloride?

  7. Review from Lessons 5 & 6 • Solid barium carbonate can be prepared in the lab by reacting barium chloride with sodium carbonate. What mass of barium chloride must be used if 9.85g of barium carbonate is desired? • BaCl2 + Na2(CO3)  BaCO3 + 2NaCl

  8. Lesson #8 – Kinetic Molecular Theory of Gases

  9. Key Terms • Atm • Mm Hg • Kilopascals • Atmospheric pressure • Kinetic molecular theory of gases

  10. Kinetic Molecular Theory of Gases • Kinetic = ________ • Molecular = _____________ • So the KMT is the _________________ • _________________ • _________________ • _________________ • _________________

  11. Kinetic Molecular Theory of Gases • Solids move ___________________ • Eg. Hot pan vs. cold pan • Liquids ____________ • ___________________ • ___________________ • Gases move in a ________________________________________ • ____________________

  12. Solids and Liquids http://www.youtube.com/watch?v=ynUso6rJ0rE&feature=related • Are ______________ • Have _____________ • Atoms in solids and liquids are _________ • ___________________ • ___________________ • What do you think about gases?

  13. The Gas State • Translational motion: • Gas particles travel in a ______________ until they collide with the side of the container or with another particle. • Gas particles move faster than those in liquids and solids • Gas particles will ______________________________ • ________________________– if compressed enough the forces between molecules will become strong enough to hold the gas molecules together. This is the point where a gas changes to a liquid – condensation.

  14. GASES • Gases are one of the most pervasive aspects of our environment on the Earth. We continually exist with constant exposure to gases of all forms. • The steam formed in the air during a hot shower is a gas. • The Helium used to fill a birthday balloon is a gas. • The oxygen in the air is an essential gas for life.

  15. GASES A windy day or a still day is a result of the difference in pressure of gases in two different locations. A fresh breeze on a mountain peak is a study in basic gas laws.

  16. Important Characteristics of Gases 1) ________________________________________ An external force compresses the gas sample and decreases its volume, removing the external force allows the gas volume to increase. 2) _______________________________________ When a gas sample is heated, its volume increases, and when it is cooled its volume decreases. 3) _____________________________________________ Gases flow much easier than liquids or solids. 4) __________________________________________ Gas densities are on the order of grams per liter whereas liquids and solids are grams per cubic cm, 1000 times greater. 5) _______________________________________________ Gases mix in any proportion such as in air, a mixture of many gases.

  17. Substances That Are Gases under Normal Conditions Substance Formula MM(g/mol) • Helium He 4.0 • Neon Ne 20.2 • Argon Ar 39.9 • Hydrogen H2 2.0 • Nitrogen N2 28.0 • Nitrogen Monoxide NO 30.0 • Oxygen O2 32.0 • Hydrogen Chloride HCl 36.5 • Ozone O3 48.0 • Ammonia NH3 17.0 • Methane CH4 16.0

  18. Forces Between Particles • The weaker the attractive force between molecules, _____________________________________________________ • Attractive forces are _____________________ • Attractive forces are the ____________________________________ • The strength of forces depends on ________________________________________________________________________________

  19. Attractions Between Charged Particles • Remember ionic bonding? = • Ions form very ______________, therefore this explains why ______________________________________________ • Attraction also happens between neutral molecules: remember intermolecular forces? • Polar molecules are attracted by __________________________ (eg.H20 OR SO2)

  20. Polar Molecules • Polar molecules ____________________________________ (as their bonds are not as strong as ionic) • Ethanol is ________________________________ • Hydrogen chloride _____________________

  21. What about non-polar (symmetrical) molecules? • Have temporary dipoles • __________________ • ____________________________________ • Eg. Carbon dioxide

  22. Size DOES Matter! • __________________________________________________________________________ • Eg. Methane (CH4) vs. Pentane (C5H12)

  23. Temperature • Temperature is _________________________ • Hotter substances have _____________________________________ • Cooler substances with ____________________________________________________________________________

  24. Summary • State of substance depends on ____________ • _____________________________________ • Strong = _____________________ • Weak = ___________________ • State of non-polar molecules depends on size • Smaller = ______________ • Larger = ______________________________

  25. The Kinetic Molecular Theory of Gases assumes that: • This means that individual gas molecules have virtually no volume of their own, and are extremely far apart and most of the container is empty space.

  26. The Kinetic Molecular Theory of Gases assumes that: • There are neither______________________ • ____________________________________ • Gas molecules have high __________________. They move randomly in all directions, in straight lines. • Collisions are perfectly elastic, ___________________________(think of pool balls)

  27. The Kinetic Molecular Theory of Gases assumes that: • Kinetic energy of a gas molecule is directly • _____________________________________ • The greater the temperature, _____________ • _____________________________________ • _____________________________________

  28. Gas Pressure and Volume • How are these related? • Can anyone think about some examples? • Why is this relationship so important?

  29. Gas Pressure and Volume • http://www.youtube.com/watch?v=is4J1Ml-uW8

  30. How is Pressure Calculated? • Pressure = • Pressure is usually reported using kilopascals (kPa) • A decrease in surface area can dramatically increase pressure! • Girls, think about what happens when you wear high heels!

  31. Atmospheric Pressure • __________________ is the force exerted on you by the weight of tiny particles of air (air _________________). • Air molecules are invisible, they still have weight and take up space. Since there's a lot of "empty" space between air molecules, air can be compressed to fit in a smaller ________________

  32. Atmospheric Pressure

  33. Galileo vs. Torricelli • Galileo invented a suction air pump • Torricelli, Galileo’s secretary, continued the investigation and hypothesized the use of mercury because of it’s density. • The barometer was born

  34. Units of Pressure • We used to use mm Hg • Standard atmospheric pressure (SAP) at sea level and 0 degrees is 760 mm Hg • Also SAP can be defined as 760 torr • Also atmospheres = atm = 760 torr = 760 mm Hg. • Now we used kilopascals (SI unit), where SAP is 101.3kPa.

  35. In other words…… • SAP at 0 degrees Celsius is equivalent to:

  36. The Relationship Between Pressure and Volume • As ____________________, gas molecules are forced closer together. This forces the ___________________________________ • This is known as an inversely proportional relationship. • Remember by volume, we mean the volume of the container, or _____________________________________________________________________________

  37. Enter Boyle • Boyle’s Law:

  38. Homework • Please do all the questions for Lessons 5,6, & 8. • Lab is due Wednesday • All the readings for Lessons 9 &10 • Look at the new May schedule online.

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