Asked by Anya

Is this done right?

White phosphorous, P4, spontaneously bursts into flame in Oxygen gas. if 6.5 g of white phosphorous reacts completely with oxygen to form 11.54g of a phosphorous oxide, what is the empirical formula of this oxide?

this is what i did:

total = 11.4 g , P4 = 6.5 g , therefore O2= 5.04 g

converted P4 and O2 to moles and divided by the smallest # of moles (which was moles of P4= 0.0525)

so the empirical formula would be PO3


however this isn't one of the options for the answers :S

did i do smthg wrong?

thanks for help in advance!

Answers

Answered by DrBob222
Yes, you calculated mols P4 and not P. Also, you subtracted wrong; 11.4-6.5 = 4.90
6.5/31 =about 0.2
4.90/16 = about 0.3
ratio is P1:O1.5 or P2O3 for the empirical formula.

Answered by Anya
sorry it was a typo, 11.54.

but still , you are right. 5.04 / 16 = 0.315 so answer ended up being the same in the end.

thank you !
Answered by DrBob222
You're welcome.
Answered by turtle 1
I dislike chemistry sometimes.
Answered by Pundai
YUP RIGHT
Answered by Vessaimani
yup hahaha
Answered by ds
awda
There are no AI answers yet. The ability to request AI answers is coming soon!

Related Questions