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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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- Winter '10
- Torr, mm Hg