Critical point- 72.9 Solid Liquid 67 BO 5.11 Triple point Vapour 1 A Temperature, TIK Figure 4A.8 The experimental phase diagram for carbon dioxide; note the break in the vertical scale. As the triple point lies at pressures well above atmospheric, liquid carbon dioxide does not exist under normal conditions; a pressure of at least 5.11 atm must be applied for liquid to be formed. The path ABCD is discussed in Brief illustration 4A.6. Pressure, platm 216.8 298.15 304.2

Critical point- 72.9 Solid Liquid 67 BO 5.11 Triple point Vapour 1 A Temperature, TIK Figure 4A.8 The experimental phase diagram for carbon dioxide; note the break in the vertical scale. As the triple point lies at pressures well above atmospheric, liquid carbon dioxide does not exist under normal conditions; a pressure of at least 5.11 atm must be applied for liquid to be formed. The path ABCD is discussed in Brief illustration 4A.6. Pressure, platm 216.8 298.15 304.2

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter6: Equilibria In Single-component Systems

Section: Chapter Questions

Problem 6.25E: 6.25. Phosphorus exists as several allotropes that have varying properties. The enthalpy of...

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6.25. Phosphorus exists as several allotropes that have varying properties. The enthalpy of transition from white P to red P, , is . The densities of white and red phosphorus are and , respectively. At what temperature does white phosphorus become the stable phase at of pressure? Assume the formula for phosphorus is .
Complete the following table. Calculate the vapor pressure, mm Hg, for each run. Vaporpressure, Pvapor = Pequil - Pinitial. Enter T and Pvapor from the preceding table in the following table. Complete the table by calculating the temperature in degrees Kelvin, the inverse of the temperature in degrees Kelvin, construct a graph of the natural logarithm of the measured vapor pressure,ln(Pvapor), versus1Twhere T is the average Kelvin temperature using the data from the four vapor pressure determinations.
Estimate the pressure (atm) necessary to melt ice at -10°C if the molar volume of liquid water is 18.01 mL/mol and the molar volume of ice is 19.64 mL/mol. Δ?̅ (delta S bar) for the process is 122.04 J/mol·K and you can assume that these values remain relatively constant with temperature.
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?
The melting point of water at the pressure of the interest (1 atm) is 0 oC and the enthalpyof fusion is 6 kJmol-1. The boiling point is 100 oC and the enthalpy of vaporization is40kJmol-1.Calculate ΔH and ΔS for the transformation of 5 grams of H2O (ice) from (s, -10/X oC)to H2O (g, 1000/X oC)cp (water)= 75.3 joule/mole.K. cp (ice)=36.2 joule/mole.K x=4.5
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.
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/mole
(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.
a)Draw the Naphthalene Phase Diagram[MM= 128.2[g/mol]], add the development used to obtain the different values. 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].
Calculate the heat required to bring 10.0 g CCl2F2 from -29.8 °C as a liquid to the gas phase at 10.0 °C. (molar mass = 120.91 g/mol) Cs (gas) = 0.074 kJ/mol·K ΔHvap = 20.1 kJ/mol ΔHfus = 4.14 kJ/mol
Calculate the heat required to bring 10.0 g CCl2F2 from -29.8°C as a liquid to the gas phase at 10.0°C. (molar mass = 120.91 g/mol) Cs (gas) = 0.074 kJ/mol·K ΔHvap = 20.1 kJ/mol ΔHfus = 4.14 kJ/mol
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?