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- Saturatad uater vapour at 60c°has iti pressure decrease to ncrease the volume by 10 % Keeping the temperature constant. To what pressure Should be expands.The vapour pressure of a liquid is represented by the equationlog (P/Torr) =(−1625/?)+8.750 where T is the temperature in Kelvins. Use the equation to find the vapour pressure of the liquid at 23 ℃.The standard enthalpy of vaporization (H°vap) of diethylether ((CH3CH2)2O) is 29.1 kJ/mol.The normal boiling point of diethylether is 34.5°C.Calculate the vapour pressure of diethylether at 19.0°C. (Units of pressure can be atm, torr, mmHg, Pa, kPa, bar, etc. -- units are always case sensitive)
- A solvent sublimes at a temperature of 258.4 K at a pressure of 23 mm Hg, with its enthalpies of sublimation and vaporization being 30780 and 23457 J/mol, respectively. If the normal melting temperature of the solvent is 4C and the triple point temperature is 1C, calculate: a) Enthalpy of fusion and pressure at the triple point b) Can we lyophilize if we obtain a vacuum pressure of 45 mm Hg? c) Does it follow Trouton's rule? d) Is it true that the density of the solid is greater than that of the liquid? Will the solid float in the liquid?The phase diagram of NH3 can be characterized by the following information. The normal melting and boiling points are 195.2 and 239.82 K, respectively; the triple point pressure and temperature are 6077 Paand 195.41 K, respectively. The critical point is found at 112.8 x 105 Pa and 405.5 K. Make a sketch of the P-T phase diagram (not necessarily to scale). Place a point in the phase diagram for the following conditions.State which and how many phases are present.a. 195.41 K, 9506 Pab. 195.41 K, 6077 Pac. 245.5 K, 101325 Pad. 415 K, 115000 Pae. 185.5 K, 6077 PaFor SO2 melting and boiling points are 198 K and 263 K respectively. Cp values for solid phase are 1.255 J/mol-K at 15 K and 84.185 J/mol-K for greater than 15 K. Cp values for liquid phase is 24.937 J/mol-K. For gas phase Cp = 49.769 + 4.56*10 TJ/mol-k where T is in K. Enthalpy of freezing and condensation processes are -7.402 kJ/mol and-24.937 kJ/mol respectively. Determine specific entropy of SO2 at 400 K. Image of question attached.
- is the phase diagram of sulphur. At 95.4˚C, the densities of rhombic andmonoclinic sulphur are 2.07 g cm-3and 1.96 g cm-3, whilst the enthalpy change for thephase transition from rhombic to monoclinic sulphur is 0.3 kJ mol-1. i) How many triple points are there?ii) What is the most stable form of sulphur under normal conditions?iii) Describe what happens when sulphur at 1 atm is heated from 80˚C to 200˚C.iv) Determine the volume change ΔV for the transformation from rhombic tomonoclinic sulphur.v) Estimate the pressure at which rhombic and monoclinic sulphur coexist inequilibrium at a temperature of 373 K.Compound Chemical formula Hvap (kJ⋅mol−1) Boiling point (K) Hfus(kJ⋅mol−1) chloromethane CH3Cl 21.40 249.06 6.43 water H2O 40.65 373.15 6.01 hydrogen sulfide H2S 18.67 213.60 18.67 1. Trouton's rule states that the molar enthalpy of vaporization of a liquid that does not have strong molecular interactions such as hydrogen bonding or ion‑ion attractions is given by Hvap=(85 J⋅K-1⋅ mol-1)Tb Where Tb is the normal boiling point of the liquid in kelvins. Apply Trouton's rule to estimate the value of Hvap for these compounds: chloromethane: Hvap= ? kJ/mol water: Hvap= ? kJ/mol hydrogen sulfide: Hvap = ? kJ/molIs it possible to have a homogeneous, binary liquid solution that has a higher (or lower) viscosity relative to either component?
- Prepare a phase diagram for the CO2 system using the following data: solid CO2 (dry ice) sublimes at 1 bar pressure and -78ºC. The triple point is at 5.18 bar and 56.6ºC. The critical point is at 74 bar and 31.1.ºC. The density of solid is 1.56 g/ml and of the liquid 1.11g/ml. The enthalpy of fusion is 8.34 kJ/moleThe dependence of the vapor pressure of a solid mineral on temperature is given by log (p/Torr) = 10,5916 - 1871,2/(T/K) AND FOR THE LIQUID log (p/Torr) =8,3186 - 1425,7/ (T/K). Calculate the triple point temperature and pressure of this mineral.The melting point of mercury at 1 bar is −38.87°C. The density of liquid mercury atthese conditions is 13.69?/??3 and the density of the solid phase is 14.193?/??3. Theassociated heat of fusion is 9.75?/?. Estimate the melting point of mercury under the pressureof 3540???.