Wednesday February 3, 2010 (Review for Test 7). No Bell Ringer Today Bell Ringer 2-3-10.

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Presentation transcript:

Wednesday February 3, 2010 (Review for Test 7)

No Bell Ringer Today Bell Ringer

Announcements   No announcements today.

Assignments Currently Open AssignmentPage Date Issued Date Into GradeSpeed Last Day to Turn In Notes: The Kinetic- Molecular Theory of Gases/Nature of Gases 11/201/272/3 WS: Introduction to Gases 71/211/282/4 Notes: Gases and Pressure 91/221/292/5 WS: Pressure 131/252/12/8 Notes: The Gas Laws 151/262/22/9 WS: Calculations Involving Gases 191/282/42/11

Review for Test 7 The Kinetic Molecular Theory of Gases The Nature of Gases Gases and Pressure The Gas Laws

1 The Kinetic-Molecular Theory of Matter is based upon the idea that particles of matter are always in motion.

What are the five basic assumptions of the Kinetic-Molecular Theory of Gases? 2 Gases consist of large numbers of tiny particles that are far apart relative to their size. Collisions between gas particles and between particles and container walls are elastic collisions. Gas particles are in continuous, rapid, random motion. There are no forces of attraction or repulsion between gas particles. The average kinetic energy of gas particles depends on the temperature of the gas.

3 The average kinetic energy of gas particles depends upon the ________ of the gas. temperature

4 Gas molecules are _______________ and ______________ than the molecules in liquids and solids. moving faster farther apart

5 Gas molecules will spread out and occupy their entire container because of the property of ________. expansion

6 List four materials that are fluids and four that are not. Fluids Not Fluids Any liquid or any gas. any solid

7 What is the general trend in density of a substance as it passes through its three common phases? The solid phase usually has the highest density, then the liquid phase, and the gas phase has the lowest density.

8 Which phase of matter is the most compressible, and why? The gas phase is the most compressible, because there is empty space between gas particles that can be squeezed out.

9 Which phase of matter is the least compressible, and why? The solid phase is the least compressible, because there is very little empty space between solid particles that can be squeezed out.

10 Give a good example of the diffusion of a gas. Examples would be gas particles that are bounced from one place to another by molecular motion of air molecules.

11 The force of the collisions of gas particles against the inside walls of their container is called _______. pressure

12 What are the standard conditions for gas measurements? 1 atmosphere of pressure at a temperature of 0 o C

torrs of pressure is how many atmospheres? 0.59 atm

atmospheres of pressure is how many kilopascals? 583 kPa

kilopascals of pressure is how many atmospheres? atm

× 10 3 atm of pressure is how many kPa? 2.69 × 10 5 kPa?

17 What is the value of atmospheric pressure at sea level when the temperature is 0 o C and the weather is neutral? Give your answer in five different units. 760 mm Hg = 760 torr = 1 atm = Pa = kPa

18 The pressure exerted on a 650. mL sample of oxygen gas at constant temperature is increased from atm to atm. What will the final volume of the sample be? Law? Formula Boyle’s P 1 V 1 = P 2 V 2 V 2 = 313 mL

19 A sample of oxygen gas has a volume of 660. mL at 35°C. At what temperature will its volume be 750. mL? Law? Formula Charles’V 1 /T 1 = V 2 /T 2 T 2 = 350 K

20 A sample of nitrogen gas at 46°C exerts a pressure of atm. The gas is heated to 76°C at constant volume. What will its new pressure be? Law? Formula Gay-Lussac P 1 /T 1 = P 2 /T 2 P 2 = atm

21 A sample of fluorine gas at 17°C and 1.16 atm occupies a volume of 3.86 L. What volume would this gas occupy at 66°C and atm? Law? Formula Combined P 1 V 1 /T 1 = P 2 V 2 /T 2 V 2 = 5.50 L

22 What pressure, in atmospheres, is exerted by mol of hydrogen gas in a 4.00 L container at 45°C? Law? Formula Ideal PV = nRT P = 2.87 atm

23 How many moles of oxygen gas are there if the gas has a volume of 5.60 L, a pressure of 1.75 atm, and a temperature of 35°C? Law? Formula Ideal PV = nRT n = mol