00:01
There are three gases, 8 grams of methane, 18 grams of ethane, and an unknown amount of propane.
00:07
They were all added to a 10 -liter container at 23 degrees celsius.
00:12
The total pressure in the container is 5 .50 atmospheres.
00:17
Calculate the partial pressure of each gas in the container.
00:21
So the first thing we're going to need to do is convert those 23 degrees celsius into kelvin.
00:28
So we're going to add 273 .15, and this comes out to be 296 .15 kelvin.
00:40
We're going to need that for our ideal gas law.
00:43
Our ideal gas law is pv equals nrt.
00:48
And since we're looking for pressure, we can say pressure is equal to nrt over v.
00:56
So n is the number of moles.
01:01
R is our gas constant, and in this case it's going to be 0 .08206.
01:10
And the units are liters, atmospheres, mole, kelvin.
01:17
And t is our temperature, and this is in kelvin, and v is volume and liters.
01:27
So we have everything that we need to solve this problem, except for n, the number of moles.
01:35
We were given grams.
01:37
So we have to convert everything that we were given into moles.
01:41
So we're going to start with methane or ch4.
01:45
We were told we have 8 .00 grams.
01:49
So let's convert this to moles by saying one mole equals 16 .042 grams.
01:56
So we just take 8 divided by 16 .042, and we have the number of moles, which is 0 .49 -69 moles.
02:13
Now let's take our ething.
02:16
We were told that we had 18 grams of that.
02:21
So we'll use the same ratio where we have one mole.
02:25
This time we will say it is equal to 30 .068.
02:29
So we'll say 18 divided by 30 .068, and this is 0 .59864 moles.
02:42
So now all we have to do is put everything into our equation that we have...