Calculate Molar Concentration of Nitrogen Trichloride

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The discussion revolves around calculating the molar concentration of nitrogen trichloride (NCl3) in air, which was found to be 0.0025% by mass. One participant calculated the concentration to be 2.07x10^-4 mol/dm^3, while another arrived at 2.65x10^-7 M, leading to confusion over the differing results. The calculations involved determining the mass of 1 L of air at standard temperature and pressure (STP) and using the percentage by mass to find the moles of NCl3. Participants expressed curiosity about the discrepancies in their answers and sought clarification on the methodology. The thread highlights the complexities of calculating gas concentrations from mass percentages in air mixtures.
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Homework Statement


A sample of air was collected to assess the safety level of nitrogen trichloride in the air around a swimming pool. It was found that the air contained 0.0025% by mass of nitrogen trichloride. Calculate the molar concentration of nitrogen trichloride in the sample collected.


Homework Equations





The Attempt at a Solution


I know that mole is directly proportional to volume for gas. But it's percentage by mass. I have no idea how to do this.
The answer is 2.07x10^-4 moldm^-3 .

Can anyone explain to me or give me some clues?

I know that air is a mixture and should be done differently from finding empirical formula of a compound.

Thank you
 
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I worked through it and got 2.65 * 10^-7 M, a bit off from the answer you gave. I assumed standard temperature and pressure, are you given different information in the problem?

I started by calculating the mass of 1 L of air at STP, then used % by mass to calculate mass of the NCl3, used that mass + molecular weight to find the # of moles in one liter.

I'm kinda curious to see why my answer is different and if anyone else solved the problem in a different way.
 

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