00:01
Let's start this problem by remembering what the ideal gas law is.
00:05
We sometimes call this the pivner equation.
00:09
We know the pv is equivalent to n times r t, where p is our pressure, v is our volume, n is the number of moles, r is simply a gas constant, and t is temperature.
00:24
The first thing that we need to do in this problem is find the number of moles of helium that we have present.
00:30
So the way that we're going to do that is we'll rearrange this equation to get n by itself.
00:35
We'll have n as equivalent to 13 ,800 kilopascals, multiplied by 1 atm, divided by 101 .325 kilopascals.
00:47
We'll then multiply that by 2 .3 liters, divided by 0 .0821, multiplied by 298 kelvin.
00:56
Now, if you're confused as to why we have this first fraction in our calculation, this is simply converting kilopascals into atms, which is what the ideal gas law requires.
01:10
Now, when we simplify, these fractions will have that n, our number of moles, is equivalent to 12 .8 moles of helium.
01:20
But what we want to know is we want to know the maximum number of moles of helium that can be in these balloons...