Two balloons are side by side in a room. One is filled with 2 moles of helium gas and one is filled with 2 moles of oxygen gas. They are the same size. What conditions must exist for this to be so?
2006-11-27 13:14:34 · 4 answers · asked by cetinnovations 1 in Science & Mathematics ➔ Chemistry
They must be at the same temperature and pressure because each have 12.04 x 1024 molecules/atoms
2006-11-27 13:21:24 · answer #1 · answered by Robert O 2 · 0⤊ 0⤋
PV=nRT
Volume, Temperature can all be assumed as the same
P of oxygen= n oxygen R oxygen= 2 * 48.29 = 96.58
is proportional to
P of helium = n helium R helium = 2 * 386.04 = 772.08
the helium balloon must be thicker or made of a stronger material as the pressure in this balloon is 8 times higher
2006-11-27 21:24:42 · answer #2 · answered by MrWiz 4 · 0⤊ 0⤋
The universal gas law states that P*V=n*R*T; P = pressure, V = volume, R = gas constant, n = no of moles, T = temp ºK
n is the same, V is the same (same size); They are in the same room so T is the same. R is a constant. The only thing left is P; it must also be the same in both balloons.
2006-11-27 21:24:25 · answer #3 · answered by gp4rts 7 · 0⤊ 0⤋
the temperature and the pressure in the room are two conditions that would need to exist
2006-11-27 21:23:38 · answer #4 · answered by chevy_95_z71_14 1 · 0⤊ 0⤋