Wednesday February 3, 2010 (Review for Test 7)

1. WednesdayFebruary 3, 2010(Review for Test 7)

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

6. 1 The Kinetic-Molecular Theory of Matter is based upon the idea that particles of matter are always in motion.

7. 2 What are the five basic assumptions of the Kinetic-Molecular Theory of Gases? 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. Gasparticles 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.

8. 3 The average kinetic energy of gas particles depends upon the ________ of the gas. temperature

9. 4 farther apart Gas molecules are _______________ and ______________ than the molecules in liquids and solids. moving faster

10. 5 Gas molecules will spread out and occupy their entire container because of the property of ________. expansion

11. 6 List four materials that are fluids and four that are not. FluidsNot Fluids any solid Any liquid or any gas.

12. 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.

13. 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.

14. 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.

15. 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.

16. 11 The force of the collisions of gas particles against the inside walls of their container is called _______. pressure

17. 12 What are the standard conditions for gas measurements? 1 atmosphere of pressure at a temperature of 0oC

18. 13 450 torrs of pressure is how many atmospheres? 0.59 atm

19. 14 5.75 atmospheres of pressure is how many kilopascals? 583 kPa

20. 15 23.34 kilopascals of pressure is how many atmospheres? 0.2303 atm

21. 16 2.65 × 103 atm of pressure is how many kPa? 2.69 × 105 kPa?

22. 17 What is the value of atmospheric pressure at sea level when the temperature is 0oC and the weather is neutral? Give your answer in five different units. 760 mm Hg = 760 torr = 1 atm = 101325 Pa = 101.325 kPa

23. 18 The pressure exerted on a 650. mL sample of oxygen gas at constant temperature is increased from 0.325 atm to 0.675 atm. What will the final volume of the sample be? Law?Formula Boyle’s P1V1 = P2V2 V2 = 313 mL

24. 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’ V1/T1 = V2/T2 T2 = 350 K

25. 20 A sample of nitrogen gas at 46°C exerts a pressure of 0.645 atm. The gas is heated to 76°C at constant volume. What will its new pressure be? Law?Formula Gay-Lussac P1/T1 = P2/T2 P2 = 0.706 atm

26. 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 0.950 atm? Law?Formula Combined P1V1/T1 = P2V2/T2 V2 = 5.50 L

27. 22 What pressure, in atmospheres, is exerted by 0.440 mol of hydrogen gas in a 4.00 L container at 45°C? Law?Formula Ideal PV = nRT P = 2.87 atm

28. 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 = 0.387 mol