Demonstrate your knowledge of chemical thermodynamics by doing the following:

(a) Show how the molar Gibbs' energy of a pure substance depends on temperature by sketching Gm vs. T for solid, liquid, and gas phase. Plot () , () , and () on the same axes. Mark phase transition temperatures and indicate which is the stable phase in the different regions of the plot. (Note: The plot should be generic - don't use specific numbers or chemical data.)

(b) Solvent A and solute B are combined in the liquid phase. The vapor pressure of pure B is , and the Henry's Law constant for B dissolved in A is = 3 . Sketch a plot of pB (the partial pressure of B), as a function of xB , the mole fraction of component B. (Hint: remember where the ideal and ideal-dilute solutions are on such a plot)

(c) At 1 atm, water boils at 373 K, and has a heat of vaporization of 40.7 kJ/mol. But at different pressure, the boiling point temperature changes. Explain why, and estimate the maximum temperature inside a pressure cooker that operates at 2 atm absolute pressure. (You may assume the vapH is constant)