If two balloons have the same amount of atoms. Does that mean they have the same volume?

Answer 1

It's been a while since my chemistry classes, but I'm pretty sure that for ideal gasses, it's the number of molecules, not atoms. So for example, a balloon full of 1 mol of oxygen gas (O2) and a balloon full of 1 mol of carbon dioxide (CO2) gas at the same temperature will be the same size. But obviously there are more atoms in a molecule of CO2 than in a molecule of O2, so there will be a different number of atoms in the two balloons.

Answer 2

The gas law states, PV = nRT. You've said that the "amount of atoms" is the same in both cases. Let's assume they're both monoatomic gases (like He and Ar). Then n is the same in both. But what of the other variables? You could argue that temperature is the same, but how about pressure? They would have to be the same kind of balloon (same stretchiness) to have the same pressure for the same amount of gas. Under these special conditions, their volumes will be the same. But if one gas is He and the other is N2, then you've got half as many MOLECULES of N2 as you have ATOMS of helium, so the volume of nitrogen will be half (again assuming pressure and temperature are both the same in each).

Answer 3

No. If one balloon had 30 atoms of lead and one had 30 atoms of helium (you didn't say atoms of what so I'm just trying to make a point), the lead balloon would have more volume because lead atoms are much bigger than helium ones.

Answer 4

If the balloons are at the same temperature, and they are the same type of atoms (i.e. both helium) and equal amounts of each gas are in the balloons then yes they would.

Answer 5

Let's say Balloon A contains 3 x 10^25 atoms of helium and balloon B contains the same 3 x 10^25 atoms of hydrogen.

6 x 10^23 atoms of helium ---> 1 mole of He
3 x 10^25 atoms of helium ---> (3 x 10^25)/(6 x 10^23)= 50 moles of He
1 mole of He ---> 24 dm3 of He
50 moles of He ---> 1200 dm3 of He

6 x 10^23 atoms of hydrogen ---> 1 mole of H
3 x 10^25 atoms of H ---> (3 x 10^25)/(6 x 10^23) = 50 moles of H
1 mole of H ---> 24 dm3 of H
50 moles of H ---> 1200 dm3 of H

Therefore both the volumes are the same.

P.S. I think my answer is correct; However, if I am wrong, pls correct me as I have a chem test nxt week and I don't want to get my concepts wrong. Thanks! =)

Answer 6

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Answer 7

At the same pressure and temperature and if the atoms are gas and the skins are the same and they can hold gas.

Answer 8

Identical balloons in every way, at the same temperature ..Yes.

Answer 9

Yes.
1 mole of ideal gas at 25ºC and 1 atm press contains 24.465 lt
1 mole contains 6.0225 x 10 **23 atoms (Avogadros no.)

Answer 10

It depends on the surrounding temperature.