A similar experiment to the one performed in lab was carrier out by your instructor. The data was collected and analyzed with the use of Excel. The equation fr the best fit line way y=-5532.6x+20.19. Using the equation of the best fit line, calculate the heat of vaporization and the normal boiling point (in C) of this volatile liquid. Remember for this experiment pressure is measured in kPa not atm.
I know that the heat of vaporization is 45.998 kj, but how do I calculate the normal boiling point?
Solution :-
the het of vaporization obtained = 45.998 kJ/mol
using the Clausius Clayperon equation we can calculate the normal boiling point
at normal boiling point vapore pressure is same as atmospheric pressure
formula
ln(P2/P1) = Delta Hvap / R [(1/T1)-(1/T2)]
here for the T1 and P1 use the vapore pressure and temperature value from the expeirment
and for the P2 we can use 1 atm that is atmospheric pressure and solve for the T2
R= 8.314 J per mol K
so using this equation we can solve for the normal boiling point T2
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