Use the phase diagram for CO2 to answer the following. 2. At what temperature does sublimation (at 1 atm) of CO2 occur? 3. In which phase does CO2, exist at atmospheric pressure and room temperature 4. In which phase does CO2, exist at 10 atm and -15°C? 5. Find the pressure and temperature of CO2, triple point. 6. Find the critical pressure and critical temperature of CO2. 7.What is the melting point of CO2, at 100 atm? 8. From its phase diagram, why do you think CO, is called 'dry ice"?

Use the phase diagram for CO2 to answer the following. 2. At what temperature does sublimation (at 1 atm) of CO2 occur? 3. In which phase does CO2, exist at atmospheric pressure and room temperature 4. In which phase does CO2, exist at 10 atm and -15°C? 5. Find the pressure and temperature of CO2, triple point. 6. Find the critical pressure and critical temperature of CO2. 7.What is the melting point of CO2, at 100 atm? 8. From its phase diagram, why do you think CO, is called 'dry ice"?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter9: Liquids, Solids, And Materials

Section: Chapter Questions

Problem 106QRT

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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?
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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
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 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.
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