1. Burned steel wool (pure Fe) becomes a dark comp 3.50 ound referred as iron ox
ID: 1046148 • Letter: 1
Question
1. Burned steel wool (pure Fe) becomes a dark comp 3.50 ound referred as iron oxide. By burning 8 of steel wool, 5.00 g of a final product (rust) is obtained. What is the mass percent of iron (Fe) and oxygen (O) in the produced rust? 2. How many moles of Fe and O are in 5.00 g of rust? 3. What should be the empirical formula of rust formed in this way? 4. What is the balance chemical equation of the combustion of steel wood? Based on the balanced equation, how many grams of rust will be produced from 10 kg of iron? 5.Explanation / Answer
Ans 1 :
The formula of iron rust is Fe2O3.
1 mole of the compound has 2 mole of atoms of Fe and 3 mole of atoms of oxygen
The mass of Fe in 1 mole = 2 x 55.845 = 111.69 g
The mass of O in 1 mole = 3 x 15.999 = 47.997
Molar mass of the compound = 111.69 + 47.997 = 159.69 g
Mass percent of iron = ( 111.69 / 159.69) x 100 = 69.94 %
Mass percent of oxygen = ( 47.997 / 159.69) x 100 = 30.06 %
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.