A similar experiment to the one performed in lab was carrier out by your instruc

Question

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?

Explanation / Answer

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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