The given below figure is the Gibbs free energy versus pressure plot for three phases, solid (S ), liquid (L ), and gas (G ), near the triple point for the one component system. It is known that the molar volume of the solid is greater than that of the liquid.(Followed by G vs P curve of a liquid,vapour and solid).
Which of the following options is CORRECT?
- A) P – Gas, Q- Liquid, R- Solid
- B) P – Gas, Q- Solid, R- Liquid
- C) P – Solid, Q- Liquid, R- Gas
- D) P – Solid, Q- Gas, R- Solid
The molar volume is inverse of density. If the volume of the solid is larger than the liquid, higher pressure will tend to liquify the compound. P, Q and R must be part of the chart. Solids are always colder (lower energy) than liquids at the same pressure but the negative slope of the solid/liquid line can be predicted from the density difference.
Aaron Allen Is it because of this analogy that my assumption will not work for water?
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