00:01
Hi there.
00:02
We are given the density of this unknown diatomic gas.
00:07
So that means it exists with a subscript of two.
00:11
That's what a diatomic means and it is a gas at room temperature.
00:17
And we want to calculate its molar mass.
00:20
And it gives the equation to use.
00:22
It's a form of the ideal gas law equation.
00:26
It says pressure equals density times rt over molar mass.
00:35
All right.
00:35
If we want to rearrange this for molar mass, we will multiply both sides by molar mass and divide both sides by pressure.
00:47
And this molar mass will cancel over here.
00:49
Pressure will cancel over here.
00:52
And we get the equation that tells us molar mass is equal to the density times the universal gas constant.
01:01
Are times the kelvin temperature divided by the pressure.
01:06
And we're told we are at standard temperature and pressure.
01:09
So we have all of the information to solve for molar mass.
01:14
The density we were given in the problem is 3 .164 grams per liter.
01:22
The universal gas constant that i'm going to use is the one with atmospheres in it.
01:27
So that is 0 .08, 206...