The table below shows the vapour pressures of two different pure compounds as a function of temperature. For the further progress of this exercise we first assume that the two compounds form a zeotropic mixture. Later we will assume that the two compounds are not miscible with each other (hetero-azeotrope).

TASK 1 (zeotrpic mixture):
The boiling point temperature of pure compound 1 at an overall pressure of $$p_{tot}=0.10064 MPa$$ is Show entered formula Close tooltip Close tooltip Your input contains special characters which cannot be saved. Perhaps you copied text from an external program? Remove $$K$$.
The boiling point temperature of an equimolar mixture at an overal pressure of $$p_{tot}=0.1 MPa$$ is Show entered formula Close tooltip Close tooltip Your input contains special characters which cannot be saved. Perhaps you copied text from an external program? Remove $$K$$.

TASK 2 (hetero-azeotrpic mixture):
We now assume that the sames compounds are not miscible with each other. The mixture forms a hetero-azeotrope. The hetero-azeotrope contains 1mol of compound 1 and one mol of compound 2.
The boiling point temperaure of the hetero-azeotrope at a total pressure of $$p_{tot}=0.10212506 MPa$$ is Show entered formula Close tooltip Close tooltip Your input contains special characters which cannot be saved. Perhaps you copied text from an external program? Remove $$K$$.