Monday

April 21, 2014

April 21, 2014

Posted by **Chloe** on Tuesday, April 30, 2013 at 3:52pm.

I don't know how to solve this problem either. And yes, this is the question for this problem. I even double check it. Please help.

Chloroform (CHCL3) has a normal boiling point of

61 'C and an enthalpy of vaporization of 29.24 kJ/mol. What is the value of delta Gvap (in kJ) at 61'C for chloroform?

Chemistry - DrBob222, Tuesday, April 30, 2013 at 3:39pm

I wonder if this is the real problem? Isn't delta G = zero at the boiling point? It would have made more sense to ask for dS vap at the normal boiling point. And how could you calculate dG anyway with no dSvap given?

- Chemistry -
**DrBob222**, Tuesday, April 30, 2013 at 4:01pmIf that is the problem I would answer dG = 0 since you have an equilibrium at the normal boiling point and dG = 0 at equilibrium.

- Chemistry -
**Chloe**, Tuesday, April 30, 2013 at 4:38pmdG=? . how do I start this problem?

Do I use dG= -RT*ln*K?

dG=-(0.008314 kj/k*mol) (61+ 273.15) ln (29.24)??

I tried this and it is wrong.

- Chemistry -
**DrBob222**, Tuesday, April 30, 2013 at 4:44pmThere is no "starting it" if I'm right. dG = 0 since the solution at its normal boiling point is zero. There is no calculation. delta G = zero, period.

- Chemistry -
**Chloe**, Tuesday, April 30, 2013 at 4:50pmok thank you!

- Chemistry -
**DrBob222**, Tuesday, April 30, 2013 at 4:55pmPlease follow up with my answer. I would like to know if I need to adjust my thinking.

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