11.21 Answer the following questions based on the P-T phase diagram of carbon dioxide:
(a) At what temperature and pressure can the solid, liquid and vapour phases of CO2 co-exist in equilibrium ?
(b) What is the effect of decrease of pressure on the fusion and boiling point of CO2 ?
(c) What are the critical temperature and pressure for CO2 ? What is their significance?
(d) Is CO2 solid, liquid or gas at (a) –70 °C under 1 atm, (b) –60 °C under 10 atm 15 °C under 56 atm ?
11.21 Answer the following questions based on the P-T phase diagram of carbon dioxide:
(a) At what temperature and pressure can the solid, liquid and vapour phases of CO2 co-exist in equilibrium ?
(b) What is the effect of decrease of pressure on the fusion and boiling point of CO2 ?
(c) What are the critical temperature and pressure for CO2 ? What is their significance?
(d) Is CO2 solid, liquid or gas at (a) –70 °C under 1 atm, (b) –60 °C under 10 atm 15 °C under 56 atm ?
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1 Answer
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11.21

(a) The P-T phase diagram for CO2 is shown here. O is the triple point of the CO2 phase diagram. This means that at the temperature and pressure corresponding to this point, the solid, liquid and vaporous phases of CO2 exists in equilibrium.
(b) The fusion and the boiling points of CO2 decreases with a decrease in pressure.
(c) The critical temperature and critical pressure of CO2 are 31 72.9 atm respectively. Even if it is compressed to a pressure greater than 72.9 atm, CO2 will not liquefy above the critical temperature.
(d) It can be concluded from the P-T phase diagram of CO2 that:
CO2 is gaseous at -70 , under 1 atm pr
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