The equation for the best fit line was y = - 5307.5x + 19.55. Using the equation of the best fit line, calculate the heat of vaporization and the normal boiling point (in C) of this volatile liquid. (Hint: What is the value of Pvap when liquid boils at its normal boiling point?
Heat of vaporization = -(slope x R) R= 8.314 j/mol*k
The Attempt at a Solution
The heat of vaporization is 44.127 kJ/mol, but I'm unsure of how to calculate the boiling point.
I tried using the Clausius-Clapeyron equation to find the boiling point. I got 99 C, but I'm unsure if its right. If it helps, the next problem following this problem lists several compounds and I have to find out what compound it is using the Normal Boiling point and heat of vaporization
Ethanol 78.3 C 42.4kJ/mol
iso-Propanol 82.3 C 45.4 kJ/mol
Cyclohexane 80.7 C 33.1 kJ/mol
I know that its not cyclohexane because its heat of vaporization differs from mines.