I am doing a lab writeup and am completely lost. Summary of lab itself: Calculated the vapour pressure of chloroform (TCM) across a range of temperatures (using flask apparatus). Objective is to determine the heat of vaporization of TCM using the variation of vapour pressure with temperature. Other info we are provided: Provided the Clausius-Clapeyron relation (lnP = -ΔHv/RT + C) "is independent of temperature" "C is a constant related to the entropy of vaporization" I'm supposed to: plot Pvapor vs. T, and determine the boiling temp. plot lnPvapor vs. 1/T, and determine ΔHvapor My questions: How do you calculate boiling point from this data? I am assuming it involves extrapolating and determining at what temperature Pvapor = Pbarometric ? How do you calculate ΔHvapor from this data without knowing C? That is, how are lnPvapor and 1/T related to C? (we are not given C and are supposed to determine it from the data) Help would be appreciated.