What is the partial pressure of He in a container that is at a total pressure of

Question

What is the partial pressure of He in a container that is at a total pressure of 2.33 atm and contains 1 .3 g of Ar and 3.3 g of He? a. 0.22 atm b. 0.33 atm c. 0.93 atm d. 0.52 atm e. 2.2 atm To account for the fact that the volume of a gas is directly proportional to its temperature in kelvins, it is necessary to postulate that: a. There is a distribution of molecular speeds between gas molecules b. The molecules have negligibly small volumes c. Molecules collide with each other d. On the average, molecules move faster at higher temperatures e. None of these explain this direct proportionality A helium weather balloon, when released, has a volume of 10.0 L at 27.0 degree C and a pressure of 0.872 atm. What volume, in liters, will the balloon occupy at an altitude where the pressure is 0.13 atm and the temperature is -30.0 degree C? (R = 0.0821 L.atm / mol.K) a. -76.7 L b. 1.17 L c. 1.79 L d. 54.3 L e. 85.3 L

Explanation / Answer

Q5.

Ptotal = Px+Py

for this example

Ptotal = 2.33 atm

mol of Ar = mass/MW = 1.3/39.99 = 0.0325081 mol

mol of He = mass/MW = 3.3/4 = 0.825 mol

y-He =0.825 / (0.0325081 + 0.825 ) = 0.962090

so

P-He = y-He * PTotal = 0.962090*2.33

P-H2 = 2.2416697 atm

best answer is 2.2 atm

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