Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: beethove on November 18, 2014, 09:51:10 PM
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At 136°C and atmospheric pressure, the density of TiCl4 is 5.6 g L-1. Under the same conditions, the density of gaseous N is 0.83 g L-1. Determine the molecular formula of TiCl4.
ANSWER: TiCl4
How? And the reasoning? Thanks!
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Express the density by using ideal gas equation. Calculate molecular mass with it.
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And remember that gaseous nitrogen is N2, not N!
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I did and the mole ratio is 1:1, which I guess is why the answer is TiCl4...but why do I even need to know the mole ratio between them figure out the molecular formula TiCl4?
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What mole ratio do you mean.
Confirm the molare mass from N2
You have pV = nRT, n =m/M and Rho = m/V
convert this to M =?
The same you do with the Titanium chloride. The calculated molar mass you have to split in x Ti and y Cl-.
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I just got it. Your method works. Another way (and I think what the chapter was trying to test) was that density is proportional to molar mass. So, this also solves it:
5.6 g L-1/0.83 g L-1(28.0 molar mass N2) = 189g of TiCl4
Therefore, TiCl4 is molecular formula.
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Yes correctly.
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Another way (and I think what the chapter was trying to test) was that density is proportional to molar mass.
Both approaches are perfectly equivalent and based on the same basic principles.