AP Chapter 5: Gases Name
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1 AP Chapter 5: Gases Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8.
2 AP Chapter 5: Gases 2 Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8.
3 AP Chapter 5: Gases 3 Warm-ups and problems will be collected before you take the test. Read Chapter 5 Answer the following problems in the space provided. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units. 3. Show the final answer with units. There is no credit without showing work. Pressure 1. What is the difference between a gas and a vapor? At 25 C, which of the following substances in the gas phase should be properly called a gas (G) and which should be called a vapor (V)? (a) molecular nitrogen (N 2) (b) mercury (c) water (d) methane Kinetic Molecular Theory 2. State the four assumptions of KMT of an ideal gas. 3. What happens to the peak height and curve width of the Boltzmann distribution of molecular velocities of a gas as temperature is raised? 4. Explain, in terms of the Boltzmann distribution of molecular velocities, how a liquid can evaporate below its boiling point. Diffusion/Effusion 5. What is the difference between diffusion and effusion? 6. Which gas diffuses more rapidly, nitrogen or water vapor? By what factor does the faster one diffuse? Pressure 7. Define gas pressure. 8. The atmospheric pressure at the summit of Mt. McKinley is 606 mmhg on a certain day. What is the pressure in atm and in kpa?
4 AP Chapter 5: Gases 4 Gas Laws 9. Sketch a plot of the relationships of the following gas variables: P V V V T n 10. At 46 C a sample of ammonia gas exerts a pressure of 5.3 atm. What is the pressure when the volume of the gas is reduced to one-tenth (0.10) of the original value at the same temperature? 11. Molecular chlorine and molecular fluorine combine to form a gaseous product. Under the same conditions of temperature and pressure it is found that one volume of C1 2 reacts with three volumes of F 2 to yield two volumes of the product. What is the formula of the product? Ideal Gas Equation 12. A certain amount of gas at 25 C and at a pressure of atm is contained in a glass vessel. Suppose that the vessel can withstand a pressure of 2.00 atm. How high can you raise the temperature of the gas without bursting the vessel? 13. Dry ice is solid carbon dioxide. A g sample of dry ice is placed in an evacuated 4.6-L vessel at 30 C. Calculate the pressure inside the vessel after all the dry ice has been converted to CO 2 gas. 14. A compound has the empirical formula SF 4. At 20 C, g of the gaseous compound occupies a volume of 22.1 ml and exerts a pressure of 1.02 atm. What is the molecular formula of the gas?
5 AP Chapter 5: Gases The empirical formula of a compound is CH. At 200 C, g of this compound occupies 97.2 ml at a pressure of 0.74 atm. What is the molecular formula of the compound? 16. A gas evolved during the fermentation of glucose (wine making) has a volume of 0.78 L at 20.1 C and 1.00 atm. What was the volume of this gas at the fermentation temperature of 36.5 C and 1.00 atm pressure? 17. The volume of a gas confined in a balloon is 1.3 L at a certain temperature and pressure. What is the balloon s volume if the pressure is doubled and the Kelvin temperature is reduced to one third of its original value? 18. Calculate the density of krypton at STP? 19. An elemental gas has a density of g/cm 3 at STP. Identify the gas. 20. The average distance traveled by a gas molecule between successive collisions is call mean fee path. For a given amount of gas, how does the mean free path of a gas depend on: a. density b. temperature at constant volume c. pressure at constant temperature d. volume at constant temperature e. size of the molecules
6 AP Chapter 5: Gases 6 Gas Stoichiometry 21. Methane, the principle component of natural gas, is burned in the Bunsen burner. If 15.0 moles of methane are burned, what is the volume of carbon dioxide produced at 23 o C and atm? 22. Dissolving 3.00 g of an impure sample of calcium carbonate in hydrochloric acid produced L of carbon dioxide (measured at 20.0 C and 792 mmhg). Calculate the percent by mass of calcium carbonate in the sample. 23. The volume of a sample of pure HC1 gas was 189 ml at 25 C and 108 mmhg. It was completely dissolved in about 60 ml of water and titrated with a NaOH solution; 15.7 ml of the NaOH solution were required to neutralize the HC1. Calculate the molarity of the NaOH solution. Dalton s Law 24. A sample of air contains only nitrogen and oxygen whose partial pressures are 0.80 atm and 0.20 atm respectively. Calculate the mole fraction of each gas. 25. A sample of zinc metal reacts completely with an excess of hydrochloric acid: Zn(s) + 2HCl(aq) ZnCl 2(aq) + H 2(g) The hydrogen gas produced is collected over water at 25.0 C. The volume of the gas is 7.80 L, and the pressure is atm. Calculate the amount of zinc metal in grams consumed in the reaction. (Vapor pressure of water at 25 o C is 23.8 mmhg.)
7 AP Chapter 5: Gases 7 Deviations from Ideal behavior 26. What two assumptions of KMT are not quite true for a real gas? Under what set of conditions of temperature and pressure does a real gas deviate most from an ideal gas? Explain each in terms of KMT. 27. (a) A real gas is introduced into a flask of volume V. Is the corrected volume of the gas greater or less than V? (b) Ammonia has a larger a value than neon does (see Table 5.4). What can you conclude about the relative strength of the attractive forces between molecules of ammonia and between atoms of neon? 28. Which of the following molecules has the largest a value: CH 4, F 2, C 6H 6, Ne? Explain.
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