Iron pyrite (FeS2) is the form in which much of the sulfur exists in coal. In the combustion of coal, oxygen r?
Iron pyrite (FeS2) is the form in which much of the sulfur exists in coal. In the combustion of coal, oxygen reacts with iron pyrite to produce iron(III) oxide and sulfur dioxide, which is a major source of air pollution and a substantial contributor to acid rain. What mass of Fe2O3 is produced from 63 L of oxygen at 2.67 atm and 154◦C with an excess of iron pyrite?
Answer in units of g
- JamianLv 68 years agoFavorite Answer
4FeS2 + 11O2 ========> 2Fe2O3 + 8SO2
moles O2 = 2.67 atm x 63 L / 0.08205 x (154 + 273.15K)
moles O2 = 4.80 moles
mass Fe2O3 = 4.80 moles x (2/11) x 159.69 = 139.37 grams ======> answer
- Anonymous5 years ago
IIRC, iron pyrite is FeS, not FeS2 (I don't think that Fe(IV) is a valid oxidation state of iron, either). We need to know where you ar having trouble with this problem. Please try to work on it yourself and let us know where you are getting stuck (if it's at the start, no problem, we'll help you through it). Here's a hint to get you started: start by writing the unbalanced equation for the reaction of iron pyrite and oxygen to form SO2 and Fe2O3.