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January 22, 2017
Posted by **Helpme** on Sunday, October 16, 2011 at 7:34pm.

Hi Please help verify my answer to the following question:

0.500g of pure phosphorous was burned in excess pure oxygen to give a product that has a mass of 1.145 g. What is the empirical formula of the resulting compound? By the use of a mass spectrometer the molecular mass of this compound (phosphorous oxide) was determined to be approximately 285 amu. What is it's molecular formula?

I was able to determine the empiricle formula as being PO3 (P 0.0161446 O 0.0403125)but don't know how to find the molecular mass.

Please verify my empiricle formula too because when I google formula for phosphorous oxide it tells me something different.

Please a step by step explaination for Molecular mass would be helpful as I don't have an example in my text to refer to which is why I posted here.

Best Regards

Chemistry - DrBob222, Saturday, October 15, 2011 at 11:18pm

The empirical formula is P2O5; you should go back over your calculation and find the error. Post your work if you want me to check it.

For the molecular formula, it is done this way.

empirical formula mass P2O5 = 141

molar mass = 285

285/141 = 2.02 which rounds to 2.0 so the molecular formula is two units of the empirical formula or

(P2O5)2 or P4O10.

Chemistry - Helpme, Sunday, October 16, 2011 at 7:32pm

Here is wht I did if you can please tell me where I went wrong would be appreciated.

resulting compound phosphorous oxide mass = 1.145g

# of moles of Phosphorus = 0.500g/30.97g/mol = 0.0161446mol

# of grams of combined phosphorus oxide = 1.145g-0.500g (P) = 0.645g of oxygen

#of moles of oxygen = 0.645g/16.00g/mol = 0.0403125mol

Therefore P 0.0161446 O 0.0403125 which divided into the smallest = P1 and O2.4969 which is then rounded to P1O3???? Please verify all of this against the question and let me know where I'm going wrong.....

Best Regards

- Chemistry -
**DrBob222**, Sunday, October 16, 2011 at 9:08pmHere is what I did if you can please tell me where I went wrong would be appreciated.

resulting compound phosphorous oxide mass = 1.145g

# of moles of Phosphorus = 0.500g/30.97g/mol = 0.0161446mol**This step is OK.**

# of grams of combined phosphorus oxide = 1.145g-0.500g (P) = 0.645g of oxygen**This step is ok if you relabel it as grams phosphorus oxide - g P = grams oxygen = 0.645g**

#of moles of oxygen = 0.645g/16.00g/mol = 0.0403125mol**This step is ok.**

Therefore P 0.0161446 O 0.0403125 which divided into the smallest = P1 and O2.4969 which is then rounded to P1O3????**This is where you are going wrong. You have P1 O 2.4969 and you should round; however, 2.4969 can't be rounded to 3 or 2. You could round it to 2.5 (and should) but you can see that P1 O 2.5 actually is P2O5 using small whole numbers. The general rule for rounding in elementary classes is to round 1.1 or so to 1 and 1.9 or so to 2 but 1:1.25 should be counted as 4:5 and 1:1.33 should be counted as 3:4. I find the easiest way to see this is to take a number like 1:2.249 and multiply both numbers by 2,3,4,5 sequentially to see if you can get small whole numbers out of it. Multiplying by 2 gives 2:4.98 and we can round that to 2:5. If we had P1 O 1.33 we would try multiplying by 2 to give 2:2.66(which CAN'T be rounded to whole numbers) so then we try multiplying by 3. That gives us 3:3.99 and we can round that to 3:4. Etc.**Please verify all of this against the question and let me know where I'm going wrong.....

Best Regards - Chemistry -
**Helpme**, Sunday, October 16, 2011 at 10:33pmThis is very helpful. I'm sure this will be reviewed in upcoming classes and understanding this information will help me be a bit ahead of the game.

Thank you very much for your help, I'm sure it wasn't an easy feast to type all this information down. Very appreciated.