Posted by richardm on October 28th, 2009
We saw how we can construct an ideal binary phase diagram (lens diagram) from our expression for the free energy of mixing of two ideal components. Our next step is to see what information this type of diagram gives us.
Solutions to Homework #7 have been posted, as well as last year’s Exam 2.
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Posted by richardm on October 26th, 2009
We developed the beginnings of an ideal binary phase diagram for a two component system that can exist in the solid and liquid phase.
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Posted by richardm on October 23rd, 2009
We explored homogeneous and heterogeneous nucleation of a solid from a liquid phase.
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Posted by richardm on October 21st, 2009
We completed two of three practice problems and then began to explore phase transitions in a qualitative manner.
A new homework was also distributed.
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Posted by richardm on October 19th, 2009
We derived the Clapeyron Equation to describe the coexistence curve for a single component system. This required a few assumptions which led us to the Clausius-Clapeyron Equation for the equilibrium between a condensed, pure phase and the vapor phase.
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Posted by richardm on October 19th, 2009
After finishing up the practice problems from last time, we took a look at phase equilibria in single component systems. This led to the construction of our first (of many) phase diagrams.
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Posted by richardm on October 14th, 2009
We looked at equilibria involving condensed phases and then began work on some practice problems. We will finish those up on Friday. Homework #6 was distributed.
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Posted by richardm on October 12th, 2009
We derived the van’t Hoff Equation for the temperature dependence of the equilibrium constant. We also saw how to write the equilibrium constant in terms of mole fractions and completed one example.
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Posted by richardm on October 9th, 2009
Using the idea of chemical potential we can up with the familiar expression for the equilibrium constant of a gas-phase reaction.
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Posted by richardm on October 7th, 2009
We took a long look at how you come up with the expression for the chemical potential of an ideal gas. This lead us to consider the mixing of ideal gases, which is completely driven by entropy.
Homework #5 has been posted on the site and hard copies will be distributed on Friday.
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