9 moles of Ammonia (NH3) are added to 50 L of H2O at a temperature of 29°C. The vapor pressure of water alone is 29.96 mmHg at 29°C. What is the vapor pressure of the Ammonia solution?

 The vapor pressure of the solution at is 29.86 mm Hg

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 : 9 moles of are dissolved in 50 L or 50000 ml of water

mass of water =  

moles of solvent (water) =

Total moles = moles of solute  + moles of solvent = 9 mol + 2778 mol = 2787  

= mole fraction of solute  

=

Thus the vapor pressure of the solution at is 29.86 mm Hg

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