Determine the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69.9 and 30.1 respectively. Given that the molar mass of the oxide is 159.8 g mol^(-1).

Determine the molecular formula of an oxide of iron in which the mass

1.	Determine the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69.9 and 30.1 respectively. Given that the molar mass of the oxide is 159.8 g mol^(-1).
Answer» Solution :For calculation of empirical FORMULA, Empirical formula (`Fe_2O_3`) mass = (`2 XX 55.85) + (3 xx 16.00) = 159.7 g mol^(-1)` `N=("Molar mass")/("Empirical formula mass") = 159.8/159.7=1` Here, MOLECULAR formula of the given OXIDE = `Fe_(2)O_(3)`.