Justify your answer: cO, Phase Diagramnot to scalesolidsupercritical fluidliquidPor critical pressurecritical point73 atmPtptriple pointgaseous5.11 atmTipcriticalTar' temperature-56.4°C31.1°CTemperatureWhat phase of carbon dioxide exists at -120°C at 1 Atm? At 80°C and 100 Atm? Justify your answer.Pressure DSupercriticalfluid217.7Critical pointNormal meltingpointSolid. Normal boilingpointLiquid1GasA6.0 x 10-3BTriple point100 374.40.0098What phase of water exists at 100°C and 5 Atm? At 200°C and 1 Atm? Justify your answer.Pressure (atm)

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Answered: What phase of carbon dioxide exists at…

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter87: Steam Distillation

Section: Chapter Questions

Problem 2P

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Dichloromethane, CH2Cl2,is widely used as a degreaser and paint stripper. Its vapor pressure is 381.0 mm Hg at 21.9C and 465.8 mm Hg at 26.90C. Estimate (a) its heat of vaporization (Hvap). (b) its normal boiling point.
The following data are the equilibrium vapor pressure of limonene, C10H16, at various temperatures. (Limonene is used as a scent in commercial products.) (a) Plot these data as ln P versus 1/T so that you have a graph resembling the one in Figure 11.13. (b) At what temperature does the liquid have an equilibrium vapor pressure of 250 mm Hg? At what temperature is it 650 mm Hg? (c) What is the normal boiling point of limonene? (d) Calculate the molar enthalpy of vaporization for limonene using the Clausius-Clapeyron equation.
A 1.50-g sample of methanol (CH3OH) is placed in an evacuated 1.00-L container at 30 C. (a) Calculate the pressure in the container if all of the methanol is vaporized. (Assume the ideal gas law, PV = nRT.) (b) The vapor pressure of methanol at 30 C is 158 torr. What mass of methanol actually evaporates? Is liquid in equilibrium with vapor in the vessel?
ln(Pvap) = −[(∆Hvap)/(R)]([ 1/(T)]) + C (Note that Pvap is the vapour pressure in atm.)The following graph was obtained for a pure volatile liquid substance. Determine the enthalpy of vaporization for this substance.ΔHvap =
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
Consider the following equation: ln(Pvap) = −[(∆Hvap)/(R)]([ 1/(T)]) + C (Note that Pvap is the vapour pressure in atm.) The following graph was obtained for a pure volatile liquid substance. (See attached graph/image) Determine the enthalpy of vaporization for this substance.
The following information is given for bismuth at 1atm: boiling point = 1627 °C Hvap(1627 °C) = 172 kJ/mol melting point = 271 °C Hfus(271 °C) = 11.0 kJ/mol specific heat solid= 0.126 J/g°C specific heat liquid = 0.151 J/g°C What is H in kJ for the process of freezing a 35.8 g sample of liquid bismuth at its normal melting point of 271 °C.________ kJ
The fragment of H2O phase diagram is shown. A) What transition (e.g. liquid--> solid, solid-->gas... or none) would be observed when a sample of H2O initially at 0.003atm and -5 C is heated at constant pressure to 50 C? B) How many phases coexist at point with T = 100 oC and p = 1 atm?
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 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???.
The vapor pressure, ?,P, of a certain liquid was measured at two temperatures, ?.T. The data is shown in the table. T (K) P (kPa) 325 3.53 775 6.53 Keep the pressure units in kilopascals. If you were going to graphically determine the enthalpy of vaporizaton, Δ?vap,ΔHvap, for this liquid, what points would you plot? To avoid rounding errors, use three significant figures in the ?x‑values and four significant figures in the ?y‑values. point 1: ?=x= point 1: ?=y= point 2: ?=x= point 2: ?=y= Determine the rise, run, and slope of the line formed by these points. rise=rise= run=run= slope=slope= What is the enthalpy of vaporization of this liquid?

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