Perhaps, we should redo the problem using molar quantities:
PCl_3(l) + 1/2O_2(g) rarr ""^(-)O-P^(+)Cl_3(l)PCl3(l)+12O2(g)→−O−P+Cl3(l)
"Moles of phosphorus trichloride"Moles of phosphorus trichloride == (194*g)/(137.33*g*mol^-1)194⋅g137.33⋅g⋅mol−1
=1.41*mol=1.41⋅mol
And thus we would get "1.41 moles of phosphoryl chloride"1.41 moles of phosphoryl chloride ==
=1.41*molxx153.33*g*mol^-1=??=1.41⋅mol×153.33⋅g⋅mol−1=??.
Phosphorus trichloride has a normal boiling point of 76.176.1 ""^@C∘C; pockle3 boils at 105.8105.8 ""^@C∘C. Of course, both liquids would have vapour pressures, but the question has been poorly proposed.
"Pockle3"Pockle3 has a density of 1.65*g*mL^-11.65⋅g⋅mL−1
"Volume"Volume -=≡ "Mass"/"Density"MassDensity
"Volume"Volume == (216.2*g)/(1.65*g*mL^-1)=131*mL216.2⋅g1.65⋅g⋅mL−1=131⋅mL.
