Answer:
The solution is not ideal.
The relative strengths of the solute-solvent interactions are greater compared to the solute-solute and solvent-solvent interactions
Explanation:
The total vapor pressure is the sum of the partial pressures of water and methanol, and they are calculated by the Raoult´s law equation:
Pₐ = Xₐ Pºₐ, where Pₐ is the partial pressure of component A
Xₐ is the molar fraction of A
P⁰ₐ is the pressure of pure A
So lets calculate the partial pressures of methanol and water and compare them with the given total vapor pressure of solution:
X H2O = 0.312 ⇒ X CH3OH = 1 - 0.312 = 0.688
PH2O = 0.312 x 55.3 torr = 17.3 torr
PCH3OH = 0.688 x 256 torr = 176.1 torr
Ptotal = PH2O + PCH3OH = 17.3 torr + 176.1 torr = 193.4 torr
This pressure is less than the experimental value of 211 torr. So the solution is not ideal. The relative strength of the solute-solvent interactions are greater than the solute-solute and solvent-solvent interactions.
The reason for this is the presence of hydrogen bonding between methanol and water.
Fluorine needs one electron to fill its orbital shell. It needs 8 valence electrons
