Ncert Exercises & Solutions

11.16: 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 ${CO}_{2}$ coexist in equilibrium?

(b) What is the effect of the decrease of pressure on the fusion and boiling point of ${CO}_{2}$ ?

(d) Is ${CO}_{2}$ solid, liquid or gas at (i) –70 °C under 1 atm, (ii) –60 °C under 10 atm, (iii) 15 °C under 56 atm?

The P-T phase diagram for ${CO}_{2}$ is shown in the figure.

(a) The solid, liquid and vaporous phases of CO $_{2}$ co-exist in equilibrium at its triple point. We can see from the phase diagram that the triple point of CO $_{2}$ is –56.6 °C at 5.11 atm pressure.

(b) With a decrease in pressure, there is a decrease in the fusion and boiling points of CO $_{2}$ .

(c) The critical temperature and critical pressure of CO $_{2}$ are 31.1°C and 73 atm respectively. When any gas is compressed to a pressure greater than critical pressure, it does not liquefy above the critical temperature.

(d) It can be seen from the P-T phase diagram of CO $_{2}$ that:

(i) CO $_{2}$ is gaseous at –70°C, under 1 atm pressure.

(ii) CO $_{2}$ is solid at –60°C, under 10 atm pressure.

(iii) CO $_{2}$ is liquid at 15°C, under 56 atm pressure.

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