The vapor pressure of anthracene can be described by the following equation, with parameters given in the table provided; the parameters are valid from 496 to 614 K. Determine the heat of vaporization at a temperature of 530 K by considering temperatures + 5 K from the target. Report your answer in units of kJ/mol. B log10 (P [bar]) = %3D - T[K]+C Anthracene
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- (a) Temperature dependence of the vapor pressure of ethylene log p (mm Hg) = - 834.13 / T + 1.75 log T - 8.375 x 10-3 T + 5.3234 , which gives the temperature dependence of the molar enthalpy of vaporization derive the equation. (b) Calculate the molar enthalpy of evaporation at -103.9 oC, the normal boiling point of ethylene. Note: Use the equation that gives the temperature dependence of ΔHvap= a + bT + cT2+ ….enthalpy.The 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.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/mol
- The vapor pressure of a substance at 20.0 °C is 58.0 kPa and its enthalpy of vaporization is 32.7 kJ mol-1. Estimate the temperature at which its vapor pressure is 66.0 kPa.Assume that the temperature of the breath of a human being is 35 ° C and its relative humidity is 95% after leaving the mouth, will the exhale become visible at 10 ° C air temperature, in other words will there be be condensation? prove your statement with calculations. The vapor pressure of water at 35 ° C is 5.62 kPa (100% relative humidity) and its enthalpy of vaporization is 44 kJ/mol.The vapor pressure of 1-chlorotetradecane at several temperatures are tabulated below. T (ºC) P∗ mm Hg 98.5 1 131.8 5 148.2 10 166.2 20 199.8 60 215.5 100 Use your graph in excel to fit the data using the appropriate curve type. Based on a fit of all the data, what is a better estimate for the value of the vapor pressure at 185ºC?
- Using the data below, determine the heat of vaporization (in kJ/mol) of V by plotting the data in the correct format. Remember that the slope of the plot should be equal to the heat of vaporization divided by the gas constant.The latent heat of fusion of water at 0Cis 6.025 kJ/mol and the molar heat capacities (Cp,m) of water and ice are 75.3 and 37.7 J K-1 mol-1, respectively. The Cp values can be taken to be independent of temperature. Calculate H for the freezing of 1 mol of supercooled water at -10.0C.The temperature dependence of the vapor pressure of solid sulfur dioxide can be approximately represented by the relation log(P/Torr) = 10.5916 − 1871.2/(T/K) and that of liquid sulfur dioxide by log(P/Torr) = 8.3186 − 1425.7/(T/K). Estimate the temperature and pressure of the triple point of sulfur dioxide
- A cylinder containing ethanol is submitted to a certain pressure. At a temperature of 273 K, when the applied pressure is 1.0 atm, the vapor pressure of the ethanol is 1.25 kPa. Considering that the molar volume of ethanol at 273 K is 1.22 x 10-2 dm3/mol, calculate the vapor pressure of ethanol when the pressure on the liquid reaches 4.00 MPa.a)Draw the Naphthalene Phase Diagram[MM= 128.2[g/mol]] Numerically indicate your triple point, and sketch the vapor, liquid and solid zones, with the following information: -The critical point of naphthalene occurs at 300 [° C] and 13.15 [atm] -The fusion enthalpy is 16.9 [kJ / mol]. Also, consider that the densities of the solid and the liquid at the triple point temperature are: Ps=249[kg/m3] and Pl=1162[kg/m3]respectively. The solid vapor curve has been parameterized as: Ln P=-8600/T + 30.69 Where the pressure is in [Pa] and the temperature in [K] b) Determine the number of degrees of freedom in: an area with no curves, an equilibrium line, and at the triple point.a)Draw the Naphthalene Phase Diagram[MM= 128.2[g/mol]] Numerically indicate your triple point, and sketch the vapor, liquid and solid zones, with the following information: -The critical point of naphthalene occurs at 300 [° C] and 13.15 [atm] -The fusion enthalpy is 16.9 [kJ / mol]. Also, consider that the densities of the solid and the liquid at the triple point temperature are: Ps=249[kg/m3] and Pl=1162[kg/m3]respectively. The solid vapor curve has been parameterized as: Ln P=-8600/T + 30.69 Where the pressure is in [Pa] and the temperature in [K] b) Determine the number of degrees of freedom in: an area with no curves, an equilibrium line, and at the triple point. Just need the B :3