Question #c6f97

1 Answer
Mar 24, 2017

Answer:

You do realize that neither #PCl_3# nor #"pockle3"# are room temperature gases don't you? You could easily find the density of liquid #POCl_3#, so your given volume is INCORRECT.

Explanation:

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#.