Answer the following questions based on the $P-T$ phase diagram of $CO _{2}$
$(a)\;CO _{2}$ at $1\; atm$ pressure and temperature $-60\,^{\circ} C$ is compressed isothermally. Does it go through a llquid phase?
$(b)$ What happens when $CO _{2}$ at $4\; atm$ pressure is cooled from room temperature at constant pressure?
$(c)$ Describe qualitatively the changes in a given mass of solid $CO _{2}$ at $10 \;atm$ pressure and temperature $-65\,^{\circ} C$ as it is heated up to room temperature at constant pressure.
$(d)\;CO_{2}$ is heated to a temperature $70\,^{\circ} C$ and compressed isothermally. What changes in its properties do you expect to observe?
Answer the following questions based on the $P-T$ phase diagram of $CO _{2}$
$(a)\;CO _{2}$ at $1\; atm$ pressure and temperature $-60\,^{\circ} C$ is compressed isothermally. Does it go through a llquid phase?
$(b)$ What happens when $CO _{2}$ at $4\; atm$ pressure is cooled from room temperature at constant pressure?
$(c)$ Describe qualitatively the changes in a given mass of solid $CO _{2}$ at $10 \;atm$ pressure and temperature $-65\,^{\circ} C$ as it is heated up to room temperature at constant pressure.
$(d)\;CO_{2}$ is heated to a temperature $70\,^{\circ} C$ and compressed isothermally. What changes in its properties do you expect to observe?
(a) No
(b) It condenses to solid directly.
(c) The fusion and boiling points are given by the intersection point where this parallel line cuts the fusion and vaporisation curves.
(d) It departs from ideal gas behaviour as pressure increases.
At $1\; atm$ pressure and at $-60^{\circ} C , CO _{2}$ lies to the left of $-56.6^{\circ} C$ (triple point C ) Hence, it lies in the region of vaporous and solid phases.
Thus, $CO_2$ condenses into the solid state directly, without going through the liquid state.
At $4 \;atm$ pressure, $CO _{2}$ lies below $5.11\; atm$ (triple point C ). Hence, it lies in the region of vaporous and solidphases. Thus, it condenses into the solid state directly, without passing through the liquid state.
When the temperature of a mass of solid $CO _{2}$ (at 10 atm pressure and at $-65^{\circ} C$ ) is increased, it changes to the liquid phase and then to the vaporous phase. It forms a line parallel to the temperature axis at 10 atm. The fusion and boiling points are given by the intersection point where this parallel line cuts the fusion and vaporisation curves.
If $CO _{2}$ is heated to $70^{\circ} C$ and compressed isothermally, then it will not exhibit any transition to the liquid state. This is because $70^{\circ} C$ is higher than the critical temperature of $CO _{2} .$ It will remain in the vapour state, but will depart from its ideal behaviour as pressure increases.
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