What I Can DoConstructing a Phase Diagram: In this activity you will draft a phase diagrambased on the specifications on a separate sheet of paper.Visualize a substance with the following points on the phase diagram: a triple pointat 0.05 atm and 150 K; a normal melting point at 175 K; a normal boiling point at350 K; and a critical point at 2.0 atm and 450 K. The solid liquid line is “normal"(meaning positive sloping).For this, complete the following:1. Roughly sketch the phase diagram, using units of atmosphere and Kelvin. Labelthe area 1, 2, and 3, and points T and C on the diagram.2. Describe what one would see at pressures and temperatures above 2.0 atm and450 K.3. Describe the phase changes from 50 K to 250 K at 1.5 atm.4. What exists in a system that is at 1 atm and 350 K? 5. What exists in a systemthat is at 1 atm and 175 K?

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Answered: Constructing a Phase Diagram: In this…

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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Sketch a well-labelled typical phase diagram for a pure substance, and label all regions appropriately.
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].
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The normal boiling point of liquid pentane is 309 K. Assuming that its molar heat of vaporization is constant at 26.8 kJ/mol, the boiling point of C5H12 when the external pressure is 1.36 atm is K. Please provide only typed answer solution no handwritten solution needed allowed
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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.
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

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