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Question -

(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 1
(d) Is CO2 solid, liquid or gas at (a) – 70 °C under 1 atm (b) – 60 °C under 10 atm (c) 15°C under 56 atm?



Answer -

(a) At the triple point, temperature = – 56.6 °C and pressure = 5.11atm.
(b) Both the boiling point and freezing point of CO2 decreaseif pressure decreases.
(c) The critical temperature and pressure of CO2 are 31.1°C and73.0 atm respectively. Above this temperature, CO2 will notliquefy/even if compressed to high pressures.
(d) (i) The point (- 70 °C, 1.0 atm) lies in the vapour region. Hence, CO2 isvapour at this point.
(ii) The point (- 60 °C, 10 atm) lies in the solid region. Hence, CO2 issolid at this point.
(iii) The point (15 °C, 56 atm) lies in the liquid region. Hence, CO2 isliquid at this point.

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