00:01
Hello students, so the question is to calculate the enthalpy of vaporization of water by the given data.
00:08
So, here the vapor pressure at p1 is equal to 55 .3 torr which is at temperature 40 degrees celsius and at 80 degrees celsius the vapor pressure of the water is p2 and it is equal to 355 torr.
00:23
So, first we need to convert the temperatures into the kelvin.
00:27
So, here the t1 is equal to 40 degrees celsius to convert it into kelvin we need to add 273 .15 and it is equal to 313 .15 kelvin and the t2 over here is 80 degrees celsius.
00:48
So, by adding 273 .15 and it is equal to 353 .15 kelvin.
00:59
So, by now by using the clausius -clapeyron equation which is ln of p2 upon p1 is equal to minus of delta h of vaporization divided by r which is the gas constant multiplied by 1 by t2 minus 1 by t1.
01:31
So, by putting the values of p2, p1 and r which is over here is the universal gas constant and it is equal to 8 .314 joule per mole per kelvin and by putting the value of 1 upon t2 and 1 upon t1 we will get the delta h of vaporization...