3 L and at a temperature of 32C exerts a pressure 47 atm Calculate the number

3 l and at a temperature of 32c exerts a pressure 47

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A sample of nitrogen gas kept in a container of volume 2.3 L and at a temperature of 32°C exerts a pressure 4.7 atm. Calculate the number of moles of gas present. (8 points) PV=nRT 4.7 x 2.3=n x .0821 x 305K 1 Copyright © 2017 by Thomas Edison State University . All rights reserved.
10.81=n x 25.04 n=.43moL of N gas present. (Reference: Chang 5.31) 5.What volume will 5.6 moles of sulfur hexafluoride (SF6) gas occupy if the temperature and pressure of the gas are 128°C and 9.4 atm? (8 points) 6. A gas-filled balloon having a volume of 2.50 L at 1.2 atm and 25°C is allowed to rise to the stratosphere (about 30 km above the surface of Earth), where the temperature and pressure are –23°C and 3.00 × 10 –3 atm, respectively. Calculate the final volume of the balloon. (8 points) (Reference: Chang 5.35) (1.2atm x 2.50L) (298K) = (3.00 x 10^-3atm x V2/250K) .0007 x 250K= 2.5175/3.00 x 10^-3 atm= 8.39 x 10^-4 = 839L 7. A 2.10-L vessel contains 4.65 g of a gas at 1.00 atm and 27.0°C. (a) Calculate the density of the gas in grams per liter. (b) What is the molar mass of the gas? (10 points) PV/RT=1.00 x 2.10/.08206 x 300=.0853 4.56g/.0853mol= 54.5g/mol 54.5 x 1.00/.08206 x 300= 2.21g/L (Reference: Chang 5.47) 8. A certain anesthetic contains 64.9 percent carbon, 13.5 percent hydrogen, and 21.6 percent oxygen by mass. At 120°C and 750 mmHg, 1.00 L of the gaseous compound weighs 6.90 g. What is the molecular formula of the compound? (10 points) 750mmHg/760mmHg = 0.987atm N = PV/RT = (0.987*1) / (0.0821*393.15) = 0.0306 moles 0.0306 moles = 6.90g/molecular wt Molecular wt =224.8 64.9 g C + 13.5 H + 21.6 g O = 100 g of anesthetic

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