Three balloons filled different gaseous compounds each with a volume of 22.4 l at stp.?

Question

Would they have the same mass or contain the same number of molecules?

Answer 1

same # of molecules.......duh

mass is dependant on atomic mass. 22.4 L is the amount of 1 mole, therefore, mass is one mole, or the atomic weight in grams.

Answer 2

One mole of an ideal gas fills 22.4L at STP by the ideal gas law. So, each balloon has 1 mole in there. One mole of nitrogen has a different mass compared to one mole of oxygen, but both have avogadro's # of molecules (not necessarily atoms, think O2 vs Ne). Hope this makes sense -- I graduated a chem major 10 years ago, but don't use it much anymore.

Answer 3

to make sparkling Jim's answer, at STP, one mole of any gas occupies a volume of twenty-two.4 L. So, multiplying the kind of moles X 22.4 L/mol provides the remarkable volume (112 L) you additionally can calculate this utilising the perfect gas regulation: PV=nRT At STP, P = a million atm T = 273.15 ok R = 0.0821 Latm/molK n = 5 you need to get a similar volume shown in Jim's answer.

Answer 4

neither. the different compounds have different elements which in turn have a different number of molecules resulting in a different mass. just think what the size of the balloons are when they are filled. one could be expanded to their max, while the other could only be blown only 1/2 or even less.

Answer 5

Yes. If they behave as perfect gases, equal volumes of gases have the same number of atoms/molecules at the same temperature and pressure. They would not have the same masses, however. The one with hydrogen would have 2 grams, the one with helium would have 4 grams, and the one with neon would have 20 graqms.

Answer 6

They contain the same number of molecules

Answer 7

According to the ideal gas they should have the same number of moles but not necessarily the same mass PV=nRT

Answer 8

molecules. 22.4 l of any gas at STP is defined as one mole of that gas, and thus it contains 6.02 x 10 ^ 23 particles (usually molecules).

Answer 9

PV=nRT

P1=P2=P3
V1=V2=V3
T1=T2=T3

Therfore
n1=n2=n3