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a. How many moles of helium are in the balloon? (1 point)
n= (1.00 ) (3425 ) / (0.0821) (273 ) n= 152.8 moles of Heb. After the balloon is released, it begins to rise. At the altitude when its pressure is 0.0474 atm and its temperature is 220.2 K, what is the volume of thehelium in the balloon? Assume that the force of the balloon on the gas is negligible. (1 point)V2 = [(1atm) (3425 L) (220.2 K)]/ [(0.0474 atm)(273 K)] V2= 58,282.32 L He
c. Suppose another weather balloon is inflated with 8000 L of hydrogen. Estimate its volume if it reaches the same elevation with this atmospheric pressure and temperature. (1 point)V2 = [(1atm) (8000L) (220.2 K)]/ [(0.0474 atm) (273 K)]V2= 136,133.9L H 4. Two sealed tanks each contains gas at 273 K. Tank A contains 9.00 g of argongas, and tank B contains 18.7 g of chlorine gas. a. How many moles of gas are in each tank? (2 points) nAr= 9/40 = 0.225 (mol)nCl= 18.7/(35,5) = 0.527(mol)
b. The volume of each tank is 5.00 L. Use the ideal gas equation to determine the pressure of the gas in each tank. (2 points) Pressure of argon = nRT/V = 0.225*0.082*273/5 = 1.007 atm Pressure of chlorine gas = 0.527*0.082*273/5 = 2.359 atmc. Explain why it is reasonable to treat the gases as ideal gases. Justify your answer by explaining what the macroscopic properties of the gases imply about the intermolecular forces within the gases. (1 point)Since the pressure is low and the temperature of the gases is much higher than their boiling points, it is reasonable to assume that the gases behave ideally.
d. Suppose a researcher wants to increase the non-ideal behavior of the gases. Should the researcher increase the temperature to T= 925 K, or should the researcher decrease the temperature to T= 92.5 K? Explain why each of these possibilities would or would not affect the non-ideal behavior of the gases. (1 point)