Question

Question #c6f97

Answer 1

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`.