The vapor pressure, P, of nitric acid varies with temperature as follows:
T/Celsius: 0, 20, 40, 50, 70, 80, 90, 100
P/kPa: 1.92, 6.38, 17.7, 27.7, 62.3, 89.3, 124.9, 170.9
What is the normal boiling point? What is the enthalpy of vaporization of nitric acid?
I'm guessing this has to do with the clausius-clapeyron equation: dlnP/dT = delta H/RT^2. Integrated, it's lnP = Constant - delta H/RT
I'm confused how to get that expression though. I'm pretty bad at excel. I'm not even sure if my method is correct. I just know if I get an expression from excel I can solve for the delta H vap and that I can find the normal boiling point too.
Thanks for any insight.