Pressure (not to scale) D C point Critical Supercritical fluid 72.9 atm 5.1 atm Solid I atm B Liquid O Triple point Gas -78.5 °C -56.7 °C Temperature (not to scale) 31 °C
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(i) The liquid region: In the liquid region, both temperature and pressure can vary independently. Show more…
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The phase diagram for CO2 is shown below. (7 points) Are each of the following statements TRUE OR FALSE. At 5.1 atm and -56.7°C, there is no liquid phase of CO2 possible. When the pressure is 1 atm, there is no temperature at which the liquid phase of CO2 exists. CO2 is a gas under normal conditions of temperature and pressure. Movement across a boundary line corresponds to a phase change. When the pressure is 4 atm and the temperature is more than -56.7 degrees Celsius, CO2 exists as a solid. Liquid CO2 is more dense than solid CO2 CO2 can never boil at atmospheric pressure (1 atm)
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Given the following data about $\mathrm{CO}_{2}$ : triple point: $-57^{\circ} \mathrm{C}, 5.11 \mathrm{~atm}$ critical point: $31^{\circ} \mathrm{C}, 73$ atm sublimes at $-78.5^{\circ} \mathrm{C}, 1 \mathrm{~atm}$ The solid is the denser phase. (a) Construct a simplified (not to scale) phase diagram for $\mathrm{CO}_{2}$ (b) Estimate the vapor pressure of $\mathrm{CO}_{2}$ at $0^{\circ} \mathrm{C}$. (c) At 10 atm pressure and $-50^{\circ} \mathrm{C},$ is $\mathrm{CO}_{2}$ a liquid?
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