The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is chlorophyll. Calculate the vapor pressure of the solution at 25 °C when 11.79 grams of chlorophyll, C55H72MgN4O5 (893.5 g/mol), are dissolved in 153.2 grams of diethyl ether. diethyl ether = CH3CH2OCH2CH3 = 74.12 g/mol. VP(solution) = mm Hg

The vapor pressure of the solution at is 460.63 mmHg

Explanation:

As the relative lowering of vapor pressure is directly proportional to the amount of dissolved solute.

The formula for relative lowering of vapor pressure will be,

where,

= relative lowering in vapor pressure

i = Van'T Hoff factor = 1 (for non electrolytes)

= mole fraction of solute  =

Given : 11.79 g of chlorophyll  is present in 153.2 g of diethyl ether

moles of solute (chlorophyll) =

moles of solvent (diethyl ether) =

Total moles = moles of solute + moles of solvent =0.01319 + 2.067 = 2.080

= mole fraction of solute  =

Thus the vapor pressure of the solution at is 460.63 mmHg

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.

thats a little if u want the answer just look it up on google thats what i do haha : )