# 2. If pressure is constant, the relationship between temperature and volume is a. direct b. Inverse

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1 Name Unit 11 Review: Gas Laws and Intermolecular Forces Date Block 1. If temperature is constant, the relationship between pressure and volume is a. direct b. inverse 2. If pressure is constant, the relationship between temperature and volume is a. direct b. Inverse 3. One way to increase pressure on a gas is to a. decrease temperature b. increase volume c. increase the number of gas particles d. lower the kinetic energy of the gas molecules 4. How do gas particles respond to an increase in volume? in kinetic energy and decrease in temperature in kinetic energy and decrease in pressure c. increase in temperature and increase in pressure d. increase in kinetic energy and increase in temperature 5. If pressure of a gas is increased and its volume remains constant, what will happen to its temperature? c. stay the same 6. If a gases volume is decreased and pressure is constant, its temperature will c. remain the same 7. If the temperature of a gas remains constant but pressure is decreased, the volume will c. remain the same 8. Convert 2.3 atm into mmhg. a mmhg b mmhg c. 2.3 mmhg d mmhg 2.3 atm 760 mmhg = 1748 mmhg so sig.fig. = 1750mmHg 1 atm 9. Convert 6.7 liters into milliliters. a ml b ml c ml d ml 6.7 L 1000 ml = 6700 ml 1 L

2 10. The pressure of a gas is torr when its volume is ml. Calculate the pressure (in atm) if the gas is allowed to expand to ml at constant temperature. (760 torr = 1 atm) a atm b atm P 1 V 1 =P 2 V 2 (0.987 atm)(400.0 ml) = x (600.0 ml) c atm atm = x d atm 11. The volume of a gas is increased from ml to ml by heating it. If the original temperature of the gas was 25.0 C, what will its final temperature be (in C)? a. 146 C b C V 1 = V ml = ml x = K = 422 C c C T 1 T K X d. 422 C e. 695 C 12. A gas exerts a pressure of one atm at standard temperature (273.0 K). What must the temperature be adjusted to for the gas to exert a pressure of 4.00 atm? (Give your answer in C) a C b C P 1 = P 2 1 atm = 4 atm x = 1092 K or 819 C c. 819 C T 1 T 2 273K X d C 13. A quantity of gas has a volume of liters at 17.0 C and 3.00 atm of pressure. To what volume must the gas be increased for the gas to be under STP conditions? a L d. 771 L P 1 V 1 = P 2 V 2 3 atm ml = 1 atm X b L e. 797 L T 1 T K 273 K c. 706 L 706 ml = X 14. What are standard temperature and pressure conditions for gases? a. 0 C and 0 torr b. 0 K and 760 torr c C and 1 atm d. 0 C and 760 torr e. 0 C and 1 torr 15. If the volume of a confined gas is doubled while the temperature remains constant, what change (if any) would be observed in the pressure? a. It would be half as large. b. It would double. c. It would be four times as large. d. It would be 1/4 as large. e. It would remain the same. 16. A given mass of gas in a rigid container is heated from 100 C to 500 C. Which of the following responses best describes what will happen to the pressure of the gas? a. The pressure will decrease by a factor of five. b. The pressure will increase by a factor of five. c. The pressure will increase by a factor of about two. (Don t forget to convert to Kelvin) d. The pressure will increase by a factor of about eight. e. The pressure will increase by a factor of about twenty-five.

3 17. Which of the following has the most molecules? (Think PV = nrt; so n = PV n is moles a L of CH 4 at 0 C and 1.00 atm RT b L of N 2 at 0 C and 1.00 atm R and V are the same in each problem. So n = P c L of O 2 at 20 C and 1.00 atm T d L of CO 2 at 50 C and 1.25 atm e L of CO at 0 C and 1.25 atm 18. Avogadro stated that equal volumes of gases under the same conditions of temperature and pressure have equal a. numbers of molecules. b. numbers of grams. c. molar masses. d. atoms. e. speeds. 19. What volume of CH 4 at 0 C and 1.00 atm contains the same number of molecules as 0.50 L of N 2 measured at 27 C and 1.50 atm? a L b L c L d L e L P 1 V 1 = P 2 V 2 T 1 T atm V 1 = (1.50 atm)(0.50 L) 273 K 300K 20. If 3.0 L of helium at 20.0 C is allowed to expand to 4.4 L, with the pressure remaining the same, what is the new temperature? a. 702 K b. 430 K V 1 = T 1 V 2 T 2 c. 157 K 3.00L = 4.4 L d K e. -55 K 293 K T 21. At what temperature will 41.6 grams N 2 exerts a pressure of 815 torr in a 20.0 L cylinder? a. 134 K (1.07 atm)(20.0 L) = (41.6 g)( ) T 815 torr 1 atm = 1.07 atm b. 176 K g 760 torr c. 238 K K = T d. 337 K e. 400 K 22. A mixture of the gases neon and krypton is in a 2.00 liter container. The partial pressure of the neon is 0.40 atm and the partial pressure of the krypton is 1.20 atm. What is the mole fraction of neon? a Dalton Law of partial pressure. b c atm atm = 1.60 atm d e atm / 0.40 = Which of the following gases has the greatest density at 0 C and 1 atm? a. N 2 28 g/mol starting with... PV = nrt remember n = (mass / mw) b g/mol substitute and rearrange...pv = (mass/mw) RT and mass / V = mw x P / (RT) c. F 2 38 g/mol d. Ne 20 g/mol and since density = mass / V... density = mw x P / (RT) e. CO 28 g/mol So...if P, R, and T are the same, the gas with the greatest molar mass will have the greatest density.

4 24. What volume of O 2, collected at 22.0 C and 728 mmhg would be produced by the decomposition of 8.15 g KClO 3? 2KClO 3 (s) 2KCl(s) + 3 O 2 (g) a L d L b L e L c L OMIT 25. Which of the following is most likely to be a solid at room temperature? a. HF d. H 2 O b. Na 2 S e. NH 3 c. N Order the intermolecular forces (dipole-dipole, London Dispersion, ionic, and hydrogen-bonding) from weakest to strongest. a. dipole-dipole, London Dispersion, ionic, and hydrogen-bonding b. London Dispersion, dipole-dipole, hydrogen-bonding, ionic c. hydrogen-bonding, dipole-dipole, London Dispersion, and ionic d.) London Dispersion, ionic, dipole-dipole, and hydrogen-bonding e. dipole-dipole, ionic, London Dispersion, and hydrogen-bonding 27. Ammonia gas is synthesized according to the balanced equation N 2 (g) + 3H 2 (g) 2NH 3 (g) If 15.0 liters of nitrogen are reacted with an excess of hydrogen, how many liters of ammonia could be produced? Assume all gas volumes are measured at the same temperature and pressure. a L d L b L e L c L OMIT 28. A gas has a volume of 3.4 L at 25 C, what is the final temperature if the volume increases to 4.7 L? V 1 = V L = 4.7 L x = 410 K T 1 T K X 29. The initial pressure of a gas is 457 mm Hg, the final volume is 750 ml with a final pressure of 650 mm Hg. What is the initial volume of the gas? P 1 V 1 = P 2 V 2 (457 mm Hg) (V 1 ) = (650 mm Hg )( (750 L) V 1 = 1070 ml 30. A gas of 3.4 moles occupies a volume of 40.6 ml at 298 K, what is the pressure of the gas? PV = nrt (P)( L) = (3.4 moles)( atm liters/mol K) (298 K) P = 2047 atm 31. At 18 C, 34.7 grams of carbon dioxide gas creates a pressure of 613 mm Hg, what is the volume of the gas? Hint: get into the correct units before you start. PV = grt ( atm)(v) = (34.7 moles)( atm liters/mol K) (291 K) C = 12 FM 44 g/mol O 2 = 32 V = 23.4 L 44 g/mol

5 32. A 3.00 L pocket of air at sea level has a pressure of 100 atm. Suppose the air pockets rise in the atmosphere to a certain height and expands to a volume of 10.0 L. What is the pressure of the air at the new volume? P 1 V 1 = P 2 V 2 (100 atm)(3.00l) = P (10.0L) P = 30.0 atm 33. The gas in a balloon occupies 3.50 L at 300. K. At which temperature will the balloon expand to 8.50 L? V 1 = V L = 8.50 L x = 729 K T 1 T K X 34. A gas is collected by water; it contains 78.5 atm of nitrogen, atm of oxygen and atm of hydrogen. Determine the total pressure of this gas. Dalton partial law of pressure 78.5 atm atm atm = 1401 atm 35. How many moles of argon are there in 20.0 L, at 25 C and 96.8 kpa? PV = nrt (0.9556atm)(20.0 L) = (n)( atm liters/mol K) (298 K) n = moles 36. What volume will 2.00 mol of oxygen gas occupy at STP? 2.00 mol of O L = 44.8 liters O 2 1 mol 37. A weather balloon has a volume of 1750 L at 103 kpa. The balloon is released to the atmosphere. At the highest point above the ground, the pressure on the balloon is 35.0 kpa. What is the new volume of the balloon at this height? PV =P 2 V2 (103 kpa) (1750 L) = (35.0 kpa) ( x ) kpa L = x x = 5150 L 35.0 kpa 38. Find the total pressure for a mixture that contains four gases with partial pressures of 0.39 kpa, 0.53 kpa,0.73 kpa,0.72 kpa. Dalton partial law of pressure 0.39 kpa kpa kpa kpa = 2.37 kpa

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