Question Problem 1: Calculate the boiling point of water at the top of San Francisco Peak (elevation 3851 m), where the barometric pressure is 65 kPa [DvapH = 40.7 kJ/mol at the normal boiling point]. SO2(s) SO2(l) p(torr) T(K) p(torr) T(K) 1.0 177.0 33.4 209.6 10.0 195.8 100.0 225.3 Problem 2: Using the vapor pressure data provided for solid and liquid SO2 find: (a) The temperature and pressure of the SO2 triple point, (b) the heat of fusion DfusH of SO2 at the triple point. [HINT 1: Convert the pressures to bar, plot ln(p) vs 1/T for solid and liquid vapor lines and determine where they intersect. HINT 2: DfusH = DsubH – DvapH ] Problem 3: From the phase diagram for pure SiO2 (silica) provided in the figure on the next page: (a) list the names of all of the solid phases, (b) list approximate pressures and temperatures for any triple points and critical points, (c) identify the phases and transformations that occur on cooling liquid silica from 2600 to 400 oC and 2 GPa (gigapascal). Problem 4: (a) Calculate the mole fraction of glucose molecules (C6H12O6) in a 4 molal aqueous solution C6H12O6(aq). (b) Determine the concentration of solute in an aqueous solution of volume 500 cm3 that contains 23.5 g of glucose. Problem 5: (a) Calculate the molar Gibbs energy of mixing for an inert gas mixture of Argon and Neon, with mole fractions 0.8 and 0.2, respectively, at 300 K. (b) Repeat the calculation at 300K if Helium is added to the mixture so that its mole fraction is 0.2, and the ratio of the mole fractions for Argon and Neon are the same as in part(a). (c) Determine the temperature at which the molar Gibbs energy of mixing for the system in part(a) become equal to the value that you obtained for the 300K Ar/Ne/He mixture in part (b).
Question
Problem 1: Calculate the boiling point of water at the top of San Francisco Peak (elevation 3851 m), where the
barometric pressure is 65 kPa [DvapH = 40.7 kJ/mol at the normal boiling point].
| SO2(s) | SO2(l) | |||
| p(torr) | T(K) | p(torr) | T(K) | |
| 1.0 | 177.0 | 33.4 | 209.6 | |
| 10.0 | 195.8 | 100.0 | 225.3 |
Problem 2: Using the vapor pressure data provided for solid and liquid SO2 find: (a) The temperature and pressure of the SO2 triple point, (b) the heat of fusion DfusH of SO2 at the triple point. [HINT 1: Convert the pressures to bar, plot ln(p) vs 1/T for solid and liquid vapor lines and determine where they intersect. HINT 2: DfusH = DsubH – DvapH ]
Problem 3: From the phase diagram for pure SiO2 (silica) provided in the figure on the next page: (a) list the names of all of the solid phases, (b) list approximate pressures and temperatures for any triple points and critical points, (c) identify the phases and transformations that occur on cooling liquid silica from 2600 to 400 oC and 2 GPa (gigapascal).
Problem 4: (a) Calculate the mole fraction of glucose molecules (C6H12O6) in a 4 molal aqueous solution C6H12O6(aq). (b) Determine the concentration of solute in an aqueous solution of volume 500 cm3 that contains 23.5 g of glucose.
Problem 5: (a) Calculate the molar Gibbs energy of mixing for an inert gas mixture of Argon and Neon, with mole fractions 0.8 and 0.2, respectively, at 300 K. (b) Repeat the calculation at 300K if Helium is added to the mixture so that its mole fraction is 0.2, and the ratio of the mole fractions for Argon and Neon are the same as in part(a). (c) Determine the temperature at which the molar Gibbs energy of mixing for the system in part(a) become equal to the value that you obtained for the 300K Ar/Ne/He mixture in part (b).
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