00:01
So we're given that for tallywane, the boiling temperature is 100 .62 degrees celsius, and that is at normal atmospheric pressure, so at one atmosphere.
00:13
And if i convert this to kelvin, then, this is going to be 100 .62 plus 273 kelvin, which is equal to.
00:26
So we're given 373 .62 kelvin.
00:35
So boiling temperature is 373 .62 kelvin.
00:42
And the pressure at boiling is one atmosphere.
00:46
And we want to know then what is the pressure p2 at a temperature of 80 degrees celsius, which in terms of kelvin is 2.
01:00
273 plus 80.
01:06
So that then is, let's see, 273 plus 80, that is 353 kelvin.
01:16
Well, according to the clausius clipiron equation, natural log of p1 over p2 is going to be negative delta h vaporization divided by r times 1 over t1 minus 1 over t2.
01:37
And r is the ideal gas constant, which is 8 .3145 joules per mole times kelvin.
01:52
Then using the truton rule, the entropy of vaporization for most organic compounds is going to be roughly the same at 88, and that is in joules per mole kelvin.
02:23
And we also know that the entropy of vaporization is equal to the enthalpy of vaporization, delta h, divided by t, the temperature, boiling temperature, so tb.
02:51
So that means then if i know tb, i can calculate that the enthalpy here of vaporization is tb times delta s vaporization, so that then is going to be 373 .62 times 88.
03:21
And since this is in kelvin and this is in.
03:25
Joules per mole per kelvin.
03:27
I'm going to end up with jewels per mole.
03:31
And that then is equal to, let's see here, 373 .62 times 88...