Choose all that apply The substance oxygen has the following properties:normal melting point: 54.8 Knormal boiling point: 90.2 Ktriple point:critical point:1.50×103 atm, 54.4 K49.8 atm, 154.6 KA sample of oxygen at a pressure of 1.00 atm and a temperature of 106.3 K is cooled at constant pressure to a temperature of 56.9 K. Which of the following are true?Choose all that applyO One or more phase changes will occur.O The liquid initially present will vaporize.O The final state of the substance is a solid.O The final state of the substance is a liquid.O The sample is initially a gas.Submit AnswerRetry Entire Group1 more group attempt remainingPreviousNext A generic phase diagram (not to scale!) for a one component system is shown below, in which pressure in atmospheres is plotted against temperature in Kelvin. Thediagram shows the temperatures and pressures (areas) in which the solid, liquid, and gaseous phases are stable, as well as the temperatures and pressures (lines) atwhich the phases are in equilibrium with each other.BP criticalliquid1.00solidatmAP triplegasT triple T meltT boilT criticalT Kolvin• The triple point (A) is the unique temperature and pressure at which all three phases are in equilibrium with each other.• The line segment A-D, represents equibrium between the solid and liquid phases, and is often called the melting point curve. It shows how the meltingtemperature changes with pressure. The temperature at which the solid and liquid are in equilibrium at a pressure of one atmosphere is called the normalmelting point.• The line segment A-B, represents equibrium between the liquid and gaseous phases, and is often called the boiling point curve. It shows how the vaporpressure of the liquid varies with temperature and is also called the vapor pressure curve. The temperature at which the liquid and the vapor are in equilibriumat a pressure of one atmosphere is called the normal boiling point.• The vapor pressure curve terminates at the critical point (B). It is not possible to liquefy the gas, above the critical temperature. The critical pressure is thepressure required to liquefy the gas at the critical temperature. Above the critical pressure and temperature, the substance is a supercritics• The line segment A-C shows the temperatures and pressure at which the solid and gaseous phases are in equilibrium and is sometimes caPreviousNext

Melting point: Temperature below which liquid phase of molecule converts in solid phase and at this…

The substance oxygen has the following properties: normal melting point: 54.8 K normal boiling point: 90.2 K 1.50x103 atm, 54.4 K triple point: critical point: 49.8 atm, 154.6 K A sample of oxygen at a pressure of 1.00 atm and a temperature of 106.3 K is cooled at constant pressure to a temperature of 56.9 K. Which of the following are true? Choose all that apply O One or more phase changes will occur. O The liquid initially present will vaporize. O The final state of the substance is a solid. O The final state of the substance is a liquid. O The sample is initially a gas.

The substance oxygen has the following properties: normal melting point: 54.8 K normal boiling point: 90.2 K 1.50x103 atm, 54.4 K triple point: critical point: 49.8 atm, 154.6 K A sample of oxygen at a pressure of 1.00 atm and a temperature of 106.3 K is cooled at constant pressure to a temperature of 56.9 K. Which of the following are true? Choose all that apply O One or more phase changes will occur. O The liquid initially present will vaporize. O The final state of the substance is a solid. O The final state of the substance is a liquid. O The sample is initially a gas.

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 116QRT

See similar textbooks

Similar questions

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
give 5 examples of a 1 phase diagram and show its phase rule
Refer to Fig. 4A.8. Which phase or phases would you expect to be present for a sample of CO2 at: (i) 200 K and 2.5 atm; (ii) 300 K and 4 atm; (iii) 310 K and 50 atm?
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].
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 standard enthalpy of vaporization (H°vap) of ethylene glycol ((CH2OH)2) is 58.7 kJ/mol.The normal boiling point of ethylene glycol is 198.0°C.Calculate the vapour pressure of ethylene glycol at 164.5°C. (Units of pressure can be atm, torr, mmHg, Pa, kPa, bar, etc. -- units are always case sensitive)
Using the phase diagram of water, describe the process by which you can sublime 1g of ice at -10°c and at 1atm pressure to water vapour at the same temperature.
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
The enthalpy of fusion of mercury is 2.292 kJ/mol, and its normal freezing point is 234.3K with a change in molar volume of 0.517 cm3/mol on melting. At what temperature will the bottom of a column of mercury (density 13.6 g/cm3) of height 10.0m be expected to freeze?