when 0.424g of finely divided iron is burned, 0.606g reddish brown oxide is obtained. Determine the emperical formula of the oxide. Please help me solve this problem and show work. Thank you.
2007-10-03 10:42:52 · 2 answers · asked by viri4 1 in Science & Mathematics ➔ Chemistry
The increased weight of 0.606 - 0.424 = 0.182 (g) must be due to oxygen. Since Fe has atomic weight of 55.845, and Oxygen 16.00. Hence in 0.606g reddish brown oxide, 0.424g iron is 0.424/55.845 Mol = 0.00759 Mol, and 0.182g oxygen is 0.182/16.00 Mol = 0.01138 Mol. Since 0.01138/0.00759 = 1.4982 ≈ 1.5, the emperical must be Fe2O3.
2007-10-05 18:00:29 · answer #1 · answered by Hahaha 7 · 1⤊ 0⤋
you know your beginning textile Iron (fe). you know you burned it, to burn something you like Oxygen (o2). so which you would be able to assume that the a million/2 reaction is going to look something like this Fe + O2 --> something because of the fact the top product weighs greater advantageous than start up product. you may assume that the iron and oxygen formed some new compound look at your valence for oxygen and iron and you would be waiting to ensure your empirical formula for the oxide so that is Fe (some subscript) O(some subscript) B. on the grounds which you know the product, you may fill interior the blanks for B.
2016-12-28 13:22:15 · answer #2 · answered by ? 4 · 0⤊ 0⤋