Chapter_6_Problem_Sets_Questions - O O 2 How many...

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Chapter 6 Gases 39. A sample of gas has a volume of 4.25L at 25.6°C and 748 mm Hg. What will the volume of this gas be at 742 mm Hg and 26.8°C? 41. A constant-volume vessel contains 12.5g of a gas at 21°C. If the pressure of the gas is to remain constant as the temperature of the gas is raised to 210°C, how many grams of gas must be released? 43. A 12.8L cylinder contains 35.8g O 2 at 46°C. What is the pressure of this gas in atmospheres? 45. A 72.8L cylinder containing 1.85 mol He is heated until the pressure reaches 3.50 atm. What is the final temperature in degrees Celcius? 49. A gaseous hydrocarbon weighing 0.231g occupies a volume of 102mL at 23°C and 749 mm Hg pressure. What is the molar mass of this compound?
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57. What volume of O 2 (g) is consumed in the combustion of 75.6 L C 3 H 8 (g) if both gases are measured at STP? 61 Hydrogen Peroxide H 2 O 2 is used to disenfect contact lenses 2H 2 O 2 2H 2
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Unformatted text preview: O + O 2 How many milliliters of O 2 at 22°C and 752 mmHg pressure can be liberated from a 10 mL aqueous colution containing 3% H 2 O 2 by mass. Density of solution is 1.01 g mL-1 65. Which of the following actions would you take to establish a pressure of 2.00 atm in a 2.24L vessel containing 1.6g O 2 at 32°F? (a) Add 1.6g O 2 (b) Release 0.8g O 2 (c) Add 2.00g He (d) Add o.6g He 67. A 2.00L container is filled with Ar(g) at 752 mm Hg and 35°C. A 0.728g sample of C 6 H 6 vapor is added. (a) What is the total pressure in the container? (b) What is the partial pressure of each gas Q. A student collected a sample of gas in a 220mL gas bulb until the pressure reached 575 torr at 25°C. The mass of the gas is 0.299g. What is the molecular weight of the gas? PV=nRT n=m/MW MW =mRT/PV =0.299g x 0.08205L atm mol-1 K-1 x 298.16K 575/760 atm x 220/1000 L = 43.9g mol-1...
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Chapter_6_Problem_Sets_Questions - O O 2 How many...

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