Answer the following question beased on tbhe P-T phase diagram of carbon dioxide.

(a) At what temperature and pressure can the solid, liquid and vapour phases of `CO_2` co-exist is equilibrium ? (b) What is the effect of decrease of pressure on the fusion and bolling point of `CO_2` ? (c ) What are the critical temperature and pressure for `CO_2` ? What is their significane ? (d) Is `CO_2` solid, liquid or gas at (a) ` -70^@C` under 1 atm, (b) `-60^@C` under 10 atm, (c) `15^@C` under 56 atm ?

Answer the following questions based on the p-T phase diagram of carbon dioxide as shown in the figure . (i) At what temperature and pressure can the solid , liquid and vapour phases of C0_(2) co-exist in equilibrium? (ii) What is the effect of decrease of pressure on the fusion and boiling point of C0_(2) ? (iii) What are the critical temperature and pressure for C0_(2) ? what is their significance ? (iv) Is C0_(2) solid , liquid, or gas at (a) -70^(@)C under 1 atm (b) -60^(@)C under 10 atm (c) 15^(@)C under 56 atm ?

The pressure under which liquid and vapour can co-exist at equilibrium is called the

What is the effect of temperature on the vapour pressure of a liquid?

At a particular temperature and atmospheric pressure, the solid and liquid phases of a pure substance can exist i equilibrium. Which of the following term defines this temperature ?

Which points in this phase diagram represent conditions of temperature and pressure where liquid will be present ?

According to the phase diagram, what would be the effect of increasing the pressure on this substance ?

The point on the pressure temperature phase diagram where all the phases co-exist is called

A temperature at which the vapour pressure of a solid is equal to the vapour pressure of liquid is called _______.