A 44 L cylinder containing helium gas at a pressure of 37.3 atm is used to fill a weather ballon in order to lift equipment into the stratosphere. To what max pressure could a 113 L balloon be filled ?
2006-10-18 07:56:55 · 6 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
ideal gas equation PV=nRT. equate the number of moles of gas to that of balloon and gas source (cylinder) because you want total gas transfer. no helium is lost.
n=n
so, PV/RT=PV/RT
temperature is assumed constant so the PV terms for balloon and cylinder are constant. this assumption turns the ideal gas equation back to the familiar Boyle's Law.
ie, PV of cylinder= PV of balloon
pressure in the balloon is thus (cylinder pressure x cylinder volume) / (balloon volume)
ie, 44x37.3/113=14.5atmospheres
2006-10-18 08:03:11 · answer #1 · answered by Anonymous · 0⤊ 0⤋
no no no
this does not involve PV=nRT
it is Boyle's law....pressure and volume are inversely proportional
use the fact that P1V1=P2V2
plug in the 44 L and 37.2 atm for V1 and P1 and the 113 L for V2...plug and chug it to find P2
2006-10-18 08:03:07 · answer #2 · answered by Anonymous · 0⤊ 0⤋
the perfect gas equation assumes there are incredibly no interactions between the debris which make up the gas. This makes it a reliable approximation for gasses at low pressures and severe temperatures. Taking intermolecular aspects of pastime into attention makes the calculation somewhat complicated. you will in all probability could opt to treatment a collection of differential equations. Engineers detect the perfect regulation clever; by using certainty an errors of consistent with possibility some liters or kilos of hysteria could opt to no longer make lots vast distinction whilst working with agency equipment.
2016-10-19 22:57:59 · answer #3 · answered by ? 4 · 0⤊ 0⤋
44/113 x 37.3 atm
2006-10-18 08:01:43 · answer #4 · answered by Gervald F 7 · 1⤊ 0⤋
Suppose that the gas has the same temperature in the cylinder and in the balloon then (Boyle's Law):
p1*V1 = p2*V2, p2 = (p1*V1)/V2, p2 = (37.3*44)/113, p2 = 12.34 atm
2006-10-18 08:02:15 · answer #5 · answered by Dimos F 4 · 1⤊ 0⤋
first you have to find out how many moles of helium that container has in it. Use PV=nRT and I suppose at standard temperature unless the problem says differently to find the number of moles (n)
Now use PV=nRT again except now for the balloon. Use standard temperature unless directed otherwise. So you know moles, T, and V. So you can solve for P
2006-10-18 08:01:29 · answer #6 · answered by Greg G 5 · 1⤊ 0⤋