1.24g of phosphorus was burnt completely in oxygen to give 2.84g of phosphorus oxide
a. What is the empirical formula of the oxide
b. What is the molecular formula of the oxide given that 1 mole of the oxide has a mass of 284g.
a. What is the empirical formula of the oxide
b. What is the molecular formula of the oxide given that 1 mole of the oxide has a mass of 284g.
Answers & Comments
Answer:
The mass of oxygen is 2.84−1.24 = 1.60g
P O
Combining mass 1.24g 1.60g
No. of moles of atoms - 1.24/31= 0.04 1.60/16= 0.10
Ratio of moles 1 2.5
Whole numbers must be used, therefore multiply by 2
to get the empirical formula P2O
Explanation: