00:01
Hi there.
00:02
In this question, we have two balloons containing two different elements.
00:08
One balloon contains helium, and helium has an atomic mass of 4 .003 amu.
00:18
The other balloon contains argon, which has atomic mass of 39 .95 amu, which would also be their molar mass, except that would be in grams per mole.
00:35
So we know that we have equal volumes of these two gases.
00:46
They're both 1 .5 liter.
00:48
They're also at the same temperature and pressure.
00:51
So avagadro said that equal volumes of gases at the same temperature and pressure contain an equal number of particles.
01:04
So equal volumes of gases at the same temperature and pressure contain an equal number of particles.
01:10
So the first question, which balloon has the greater number of gas particles? particles, the number of gas particles are equal.
01:31
We cannot calculate the number of these without knowing the temperature and pressure, but from avagadro's principle, we do know that the number of gas particles in the two balloons must be equal because they have the same volume, the same pressure, and the same temperature.
01:52
Even without avogadro, we could conclude this thinking about the ideal gas law equation.
02:01
If pressure volume t and the universal gas constant are all the same, then n, the number of moles, must be equal between the two samples.
02:12
So the number of gas particles are equal.
02:16
Moving on, so they have equal number of particles, but argon has a greater molar mass.
02:22
So which balloon has the greater mass, the balloon with argon would have the greater mass...