00:01
All right, so in this question we're giving a mixture of methane gas and xenon gas, and we're asked to determine, and the total pressure of the gas, and we're asked to determine what the partial pressure is.
00:11
So one thing we know, one thing that can help us here, is that we know that the pressure of a is equal to the mole fraction of a times total pressure.
00:22
So we have the total pressure, so now all we need to find is the more fraction.
00:28
And then using that, we can determine what the pressure, the partial pressure of methane is.
00:34
So first, determining the moles of both these things, we have moles of ch4, which is going to be, we have 8 grams and a molar mass of 16 .042, which is going to resolve in an overall amount of 0 .49 moles.
01:03
Now, xenon is going to get the same treatment.
01:06
Where i have equally 8 grams.
01:12
Now the molar mass of this one is just quite a bit bigger.
01:15
It's going to be 131 .29 grams per mole, which is substantially larger and gives us a value of 0 .061 moles...