00:01
For this question, we'll use a form of the clausius clapperon equation, or the natural log of the vapor pressure is equal to negative delta h vaporization, divided by r, multiplied by 1 over the kelvin temperature, plus a constant.
00:22
So, if we were to take the data that's provided the kelvin temperature, converted into 1 over kelvin, the pressure and tor, take the natural log of that, then plotting the natural log of p as our y value as a function of 1 over the kelvin temperature gives us a slow people to negative delta h vaporization over r.
00:50
So the slope, as seen here, is negative 24 ,811, and that is going to be equal to negative delta h vaporization over r.
01:10
R is 8 .314.
01:16
So delta h vaporization is simply this multiplied by negative r.
01:23
And i get 206 ,000 joules per mole or 206 kilojoules per mole.
01:45
Then to calculate the temperature where the vapor pressure is one atmosphere, the normal boiling point, then i'm going to use this equation up here...