Chapter 5

# Chapter 5 - CHAPTER 5 GASES AND THE KINETICMOLECULAR THEORY...

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5-1 CHAPTER 5 GASES AND THE KINETIC- MOLECULAR THEORY 5.1 a) The volume of the liquid remains constant, but the volume of the gas increases to the volume of the larger container. b) The volume of the container holding the gas sample increases when heated, but the volume of the container holding the liquid sample remains essentially constant when heated. c) The volume of the liquid remains essentially constant, but the volume of the gas is reduced. 5.2 The particles in a gas are further apart than those are in a liquid. a) The greater empty space between gas molecules allows gases to be more compressible than liquids. b) The greater empty space between gas molecules allows gases to flow with less resistance (hindrance) than liquids. c) The large empty space between gas molecules limits their interaction, allowing all mixtures of gases to be solutions. d) The large empty space between gas molecules increases the volume of the gas, therefore decreasing the density. 5.3 The mercury column in the mercury barometer stays up due to the force exerted by the atmosphere on the mercury in the outer reservoir just balancing the gravitational force on the mercury in the tube. Its height adjusts according to the air pressure on the reservoir. On a mountaintop, the air pressure is less, so the height of mercury it balances is shorter than at sea level. 5.4 The pressure of mercury is its weight (force) per unit area. The weight, and thus the pressure, of the mercury column is directly proportional to its height. 5.5 When the mercury level in the arm attached to the flask is higher than the level in the other arm, the pressure in the flask is less than the pressure exerted in the other arm. This is an impossible situation for a closed-end manometer as the flask pressure cannot be less than the vacuum in the other arm. 5.6 The ratio of the heights of columns of mercury and water are inversely proportional to the ratio of the densities of the two liquids. 2 2 HO Hg Hg H O h d hd = 2 2 Hg H g d hx h d = = () 3 2 13.5 g/mL 10 m 1 cm 725 mmHg 1.00 g/mL 1 mm 10 m    = 978.75 = 979 cm H 2 O 5.7 P (mmH 2 O) = 2 2 Hg H g d h d = = 3 2 13.5 g/mL 10 m 1 cm 755 mmHg 1.00 g/mL 1 mm 10 m = 1019.25 = 1.02 x 10 3 cm H 2 O 5.8 a) 760 mmHg 0.745 atm 1atm = 566.2 = 566 mmHg b) 1.01325 bar 992 torr 760 torr = 1.32256 = 1.32 bar c) 365 kPa 101.325 kPa = 3.60227 = 3.60 atm

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5-2 d) () 101.325 kPa 804 mmHg 760 mmHg    = 107.191 = 107 kPa 5.9 a) 2 3 10 m 1 mm 1 atm 74.8 cmHg 1cm 760mmHg 10 m = 0.98421 = 0.984 atm b) 101.325 kPa 27.0 atm 1atm = 2735.775 = 2.74 x 10 3 kPa c) 1.01325 bar 8.50 atm = 8.6126 = 8.61 bar d) 760 torr 0.907 kPa 101.325 kPa = 6.80306 = 6.80 torr 5.10 Since the height of the mercury column in contact with the gas is higher than the column in contact with the air, the gas is exerting less pressure on the mercury than the air. 2 3 10 m 1 mm 1 torr 2.35 cm 1mmHg 10 m = 23.5 torr 738.5 torr - 23.5 torr = 715.0 torr P(atm) = 715.0 torr 760 torr = 0.940789 = 0.9408 atm 5.11 Since the height of the mercury column in contact with the gas is higher than the column in contact with the air, the gas is exerting less pressure on the mercury than the air.
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## This note was uploaded on 07/30/2011 for the course CHEM 103 taught by Professor Lewis during the Spring '08 term at Wisc Eau Claire.

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Chapter 5 - CHAPTER 5 GASES AND THE KINETICMOLECULAR THEORY...

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