When 3.40 g Na burns in air, 4.59 g oxide is formed. What is the empirical formula of the oxide?
-
Molar mass of Na is 23g
so the molar mass of the oxide is 23*4.59/3.4=31.05
if you substract 23 from 31.05 , you find 8g . this is the half of the weigth of 1 atom of oxygen. So, you have 2 atoms of Na for 1 atom oxygen and formula is Na2O
so the molar mass of the oxide is 23*4.59/3.4=31.05
if you substract 23 from 31.05 , you find 8g . this is the half of the weigth of 1 atom of oxygen. So, you have 2 atoms of Na for 1 atom oxygen and formula is Na2O