Vapor Pressure of Hg in a 10m x 10m x 3m Lab

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The vapor pressure of mercury at 25°C is 0.00185 mmHg, and a 0.1 mL drop in a 10m x 10m x 3m lab raises questions about complete evaporation and partial pressure. Given the density of mercury at 13.6 g/mL, the drop's mass is calculated, leading to an estimation of its contribution to the lab's air pressure. Despite the drop size, it is suggested that evaporation will occur over time due to the open system, preventing equilibrium with the surroundings. The normal boiling point of mercury is 630 K, indicating that vapor pressure calculations can vary significantly with temperature. Ultimately, the drop will evaporate completely, albeit at a slow rate.
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The vapor presurre of mercury is 0.00185 mmhg at 25 degree C. A single drop of Hg(0.1 mL) is spilled in a laboratory of dimensions 10m x 10m x3m. Does the entire drop evaporate? What is the partial pressure of Hg in the laboratory? (Use 13.6 g/ml for the density of Hg.) (b) The normal boiling point of mercury is 630 K. Caluculate an approimate value for vapor pressure.
 
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Wouldnt it eventually evaporate, reguardless of the size of the drop? Its just a matter of time due to the system being "Open" and therefore any evaporation does not go into equilibrium with the surroundings?
 
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