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## Homework Statement

At 1 atm of pressure a volume of 22 liters of N

_{2}gas is passed in a closed system over a boat containing Hg liquid at 100°C. The flow of N

_{2}is slow to allow the gas to become saturated with mercury. At 20°C and 1 atm, the nitrogen was found to contain 0.0647g of Hg. Calculate the vapor pressure of Hg at 100°C.

## Homework Equations

Raoult's Law (Ideal Solution):

P

_{Hg}= X

_{Hg}P°

_{Hg}

Ideal Gas Law:

PV = nRT

## The Attempt at a Solution

My endgame here is to use Raoult's Law to calculate the partial pressure of mercury. To do that, though, I will need the mole fraction X

_{Hg}and the pressure the mercury would exert if it were alone in the container P°

_{Hg}. As far as the latter goes, I suspect I can use the ideal gas law to calculate the pressure of mercury when nitrogen is not involved.

This is where I run into problems. I'm not sure how to synthesize the information given into the information I need. I could calculate a mole fraction for the system at 20°C, again via the ideal gas law, but I'm not sure how I can relate this to either P°

_{Hg}or X

_{Hg}for the same system at 100°C.

Any insight anyone can provide would be incredibly helpful and greatly appreciated.