Posted by Chloe on Tuesday, April 30, 2013 at 1:25am.
The following thermodynamic data was obtained for an unknown compound. Delta Hvap = 31.3 kj/mol and Delta S Vap= 79.7 kj/mol .Calculate the normal boiling point of this compound in Celcius..
Thank you!
Chemistry  DrBob222, Tuesday, April 30, 2013 at 12:31am
dG = dHvap  TdSvap
dG at boiling point = 0; therefore,
dHvap = TdSvap
You know dHvap and dSvap, solve for T. Check to make sure you typed the problem correctly. Check that dSvap is really in kJ/mol (or is it J/mol instead).
T will be in kelvin, convert to C.
 DrBob222,
The dSvap is J/(k*mol). I subtract the dHvap and dSvap, I got 44 Kelvin then I convert it to celsius 229.15 C. My final answer doesn't seems right. Help me please!

Chemistry  DrBob222, Tuesday, April 30, 2013 at 3:49pm
What did you subtract? I don't see a subtraction anywhere in the problem except for conversion of K to C.
dG = dH  TdS
0 = dH  TdS
dH = TdS
31300 = T*79.7
T = 31300/79.7
T = ? K
C = ?K273.15 = ?

Chemistry  Chloe, Tuesday, April 30, 2013 at 3:57pm
I realized where I made a mistake for this problem. This time, I got this one right.
Thank you so much!
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