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The equation for the best fit line was y = -4058.7x + 16.10. Using the equation of the best fit line, calculate the heat of vaporization (delta H) and the NORMAL BOILING POINT (in Celsius) of this volatile liquid.

Calculated:
dHvap = 33.7kJ/mol

----> I'm really confused on how to find the normal boiling point. I know that the pressure at normal boiling point is 101.3kPa. But I don't know where to go from there.

2 answers

Use the Clausius-Clapeyron equation. You know dHvap. Use P1 = 101.325 with T1 = unknown normal boiling point. P2 and T2 I assume are in the data/plot.
Okay thank you, since they did not give me the data plots, I'm guessing I should sketch the graph on my own.
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