00:01
All right, so to find the volume of our balloon, we're going to use the ideal gas law.
00:09
Pv is equal to nrt.
00:13
And we're going to be solving, if we want to know about volume, we're going to be dividing both sides by p to get v by itself.
00:21
And so the equation rewritten, v equals nrt over p.
00:28
Now, when we use this equation, let's look a little bit.
00:31
About the value of r because r is the universal gas constant 0 .0821 liters times atmospheres over moles times kelvin.
00:46
It's a really weird unit but it's an important one because it tells us that these are the units we need to use in our equation so if we don't have our values in these units we're gonna have to convert them to those units in order to use them.
01:02
For example, if we want to get to number of moles, we're not given the number of moles.
01:08
We're given instead the number of grams.
01:13
So we're going to have to use molar mass to convert between grams and moles.
01:20
If we have 28 .8 grams of carbon dioxide, we're going to have to use the fact that one mole of carbon dioxide has a molar mass, you can calculate it by taking a carbon and two oxygens, adding them together, of 44 .01 grams.
01:37
And that converts us into moles.
01:40
0 .654 moles...