00:01
So here we know the root mean squared speed for a gas molecule would be equaling to the square root of three times boltzmann's constant, multiplied by the temperature t divided by m, b, molar mass.
00:20
And, of course, the temperature for both gases is constant, as well as boltzman's constant is, of course, not going to change.
00:32
So we can then say that the root mean squared speed is inversely proportional to the square root of the molar mass.
00:46
And so setting up an equation, the root mean squared speed of helium divided by the root mean squared speed of xenon.
00:58
This would be equally than the square root of the molar mass of xenon divided by the molar mass of helium, divided by the molar mass of helium.
01:06
And solving, we get that the root mean squared speed of helium will be equal to then the root mean squared speed of xenon, multiplied by the square root of 131 grams per mole, divided by 4 .0 grams per mole...