Find Hg Vapor Mass in Grams at 20C Room

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Discussion Overview

The discussion revolves around calculating the mass of mercury vapor in grams at a room temperature of 20°C, based on a given vapor pressure and the dimensions of a laboratory space. The context includes both theoretical calculations and practical implications regarding air quality regulations.

Discussion Character

  • Homework-related, Mathematical reasoning

Main Points Raised

  • The initial calculation of the volume of the laboratory and the conversion to liters is presented, with the formula PV=nRT applied to find the number of moles of mercury vapor.
  • The participant expresses uncertainty about the correctness of their mass calculation, which results in 3.4 grams of mercury.
  • Another participant confirms that the setup for the calculations appears correct without checking the math.
  • A subsequent reply reiterates that the setup looks correct but questions the accuracy of the numbers used.
  • One participant simply states that the calculations look OK without further elaboration.

Areas of Agreement / Disagreement

Participants generally agree that the setup for the calculations is correct, but there is uncertainty regarding the accuracy of the numerical values and the final mass of mercury calculated.

Contextual Notes

The discussion does not resolve whether the calculated mass of mercury vapor is too high, and there are no corrections to the mathematical steps provided. The implications for air quality regulations are also noted but remain unverified.

Who May Find This Useful

Students or individuals interested in chemistry, environmental science, or air quality assessment may find this discussion relevant.

higherme
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Homework Statement


Hg is spilled in a laboratory which measures 15.2m long, 6.6m wide, and 2.4m high. Find mercury vapor in grams at 20C room. Given vapor pressure of Hg = 1.7E-6 atm.


Homework Equations

The Attempt at a Solution


Volume= 15.2*6.6*2.4 =240.768 m^3 = 240768 L
Temp = 20 + 273.15 = 293.15 K
P = 1.7E-6 atm

PV =nRT
n= PV/RT
n= (1.7E-6)(240768 L)/ (0.08206 L atm/mol K)(293.15K)
n= 0.017 mol
0.017 mol*200.6g/mol
= 3.4 g Hg

I'm not quite sure if this is how you calculate the mass of Hg. the next part of question asks if concentration of Hg exceed air quality reg. (0.050 mg Hg/m^3). According to my answer, it does exceed b/c 3.4g=3413mg/240.768m^3 = 14.2 mg Hg/m^3.

can someone check my work please, thanks in advance. I have a feeling that the mass of Hg is a bit too high...
 
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I didn't check the math, but the setup for the calculations looks correct.
 
Ygggdrasil said:
I didn't check the math, but the setup for the calculations looks correct.

are the numbers i used correct?
 
Looks OK.

--
 

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