Perhaps, we should redo the problem using molar quantities:
#PCl_3(l) + 1/2O_2(g) rarr ""^(-)O-P^(+)Cl_3(l)#
#"Moles of phosphorus trichloride"# #=# #(194*g)/(137.33*g*mol^-1)#
#=1.41*mol#
And thus we would get #"1.41 moles of phosphoryl chloride"# #=#
#=1.41*molxx153.33*g*mol^-1=??#.
Phosphorus trichloride has a normal boiling point of #76.1# #""^@C#; pockle3 boils at #105.8# #""^@C#. Of course, both liquids would have vapour pressures, but the question has been poorly proposed.
#"Pockle3"# has a density of #1.65*g*mL^-1#
#"Volume"# #-=# #"Mass"/"Density"#
#"Volume"# #=# #(216.2*g)/(1.65*g*mL^-1)=131*mL#.
