I gallon of pure phase carbon tetrachloride (CCl_4, this is a toxic solvent with

Question

I gallon of pure phase carbon tetrachloride (CCl_4, this is a toxic solvent with a vapor pressure of 0.165 atm and density of 1.59 g/mL) is spilled in a 45 m^3 room at standard temperature and pressure. Assume that CCl_4 can immediately become a gas. Using just the vapor pressure (and not the spill volume), calculate the concentration of carbon tetrachloride in the air (units = mg CCl_4 m_3 air) when the air is saturated. If all of the carbon tetrachloride in the spill becomes a gas (ignore vapor pressure), calculate the concentration of carbon tetrachloride (units = mg CCl_4/m_3 air) in the room. Which of these is the more likely scenario? Why?

Explanation / Answer

when the air is saturated with CCl4, partial pressure = vapor pressure = 0.165 atm

from gas law, PV=nRT, n/V = P/RT = 0.165/(0.0821 L.atm/mole.K* 273) =0.007362 mole/L

molar mass of CCl4 = 154, mass concentration = 0.007362*154 gm/L =1.13 g/L =1.13*1000 mg/10-3 m3 =1.13*106 mg/m3

2. when all the CCl4 becomes gas , PV=nRT, V/n = 1/(0.0821*273) =0.044616 moles/L =0.044616*154*1000mg/10-3 m3 =6.87*106 mg/L

3. There is every possibility of CCl4 evaporating and occupying the complete room is the possibility (2nd scenario).

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