- #1
aleksbooker
- 22
- 0
Hello all,
The question given is:
Mercury and many of its compounds are dangerous poisons if breathed, swallowed or even absorbed through the skin. The liquid metal has a vapor pressure of 0.00169mmHg at 24 degrees Celsius. If the air in a small room is saturated with mercury vapor, how many atoms of mercury vapor occur per cubic meter?
I can't use Clausius-Clapeyron because I only have one pressure and one temperature to work with, and I can't use PV = nRT, because I don't know how many moles of mercury I have. If I arbitrarily increase the moles, I increase the volume just as quickly, which may not affect density, but either way I don't know the concentration of moles per liter. I even considered the pressure = force/area, but that's not relevant to volume.
I'm certain the fact that the air is saturated is somehow key, but I can't find anything in my textbook that seems to address this question. What am I missing?
Thanks,
Aleks
The question given is:
Mercury and many of its compounds are dangerous poisons if breathed, swallowed or even absorbed through the skin. The liquid metal has a vapor pressure of 0.00169mmHg at 24 degrees Celsius. If the air in a small room is saturated with mercury vapor, how many atoms of mercury vapor occur per cubic meter?
I can't use Clausius-Clapeyron because I only have one pressure and one temperature to work with, and I can't use PV = nRT, because I don't know how many moles of mercury I have. If I arbitrarily increase the moles, I increase the volume just as quickly, which may not affect density, but either way I don't know the concentration of moles per liter. I even considered the pressure = force/area, but that's not relevant to volume.
I'm certain the fact that the air is saturated is somehow key, but I can't find anything in my textbook that seems to address this question. What am I missing?
Thanks,
Aleks