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Thermal Properties of Matter — Physics STD 11 Science — Question

Gujarat BoardEnglish MediumSTD 11 SciencePhysicsThermal Properties of Matter1 Mark
Question
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 $\mathrm{CO}_2$ co-exist in equilibrium ?
b. What is the effect of decrease of pressure on the fusion and boiling point of $\mathrm{CO}_2$ ?
c. What are the critical temperature and pressure for $\mathrm{CO}_2$ ? What is their significance?
d. Is $\mathrm{CO}_2$ solid, liquid or gas at (a) $-70^{\circ} \mathrm{C}$ under 1 atm , (b) $-60^{\circ} \mathrm{C}$ under $10 \mathrm{~atm}, 15^{\circ} \mathrm{C}$ under 56 atm ?
✓

Answer

The P–T phase diagram for $CO_2$ is shown in the following figure:

 The solid, liquid and vapour phase of carbon dioxide exist in equilibrium at the triple point, i.e., temprature $=-$ $56.6^{\circ} \mathrm{C}$ and pressure $=5.11 \mathrm{~atm}$. With the decrease in pressure, both the fusion and boiling point of carbon dioxide will decrease. For carbon dioxide, the critical temperature is $31.1^{\circ} \mathrm{C}$ and critical pressure is 73.0 atm . If the temprature of carbon dioxide is more than $31.1^{\circ} \mathrm{C}$, it can not be liquified, however large pressure we may apply. Carbon dioxide will be (a) a vapour, at $=70^{\circ} \mathrm{C}$ under 1 atm . (b) a solid, at $-6^{\circ} \mathrm{C}$ under 10 atm (c) a liquid, at $15^{\circ} \mathrm{C}$ under 56 atm .

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