Here's anothere chem question...btw I asked one about half an hour ago and still haven't gotten an answer...but here's my question...i REALLY REALLY need help...thank you!
A 4.43-g sample of P was burned in air to produce 10.15 g of an oxide. What's the empirical formula of this compound?
+394 Calculate the grams of oxygen 10.15g -4.43g P = 5.72g of O
Calculate the moles of phosphorus in 4.43 grams of P
0.14304 moles of P
Calculate the moles of oxygen in 5.72 grams of O
0.3575 moles of O
Divide molar masses to find the ratio
0.3575 / 0.14304 = 2.5 Phosphorus to 1 Oxygen
Multiply by 2 for integer values
P5O2
This is Phosphorus pentoxide
_7UP_
+118673 Not many people on here know about chemistry. :(
There is a couple - you might get some answers.
+394 Calculate the grams of oxygen 10.15g -4.43g P = 5.72g of O
Calculate the moles of phosphorus in 4.43 grams of P
0.14304 moles of P
Calculate the moles of oxygen in 5.72 grams of O
0.3575 moles of O
Divide molar masses to find the ratio
0.3575 / 0.14304 = 2.5 Phosphorus to 1 Oxygen
Multiply by 2 for integer values
P5O2
This is Phosphorus pentoxide
_7UP_
