Ferrophosphorus (Fe2P) reacts with pyrite(FeS2) producing iron (II) sulfide and a compound thatis 27.87 % P and 72.13 % S by mass and has a molar mass of 444.56g/mol.(A) Determine the empirical and molecular formulas of thiscompound.(B) Write a balanced chemical equation for thisreaction. Do not include phases..

Ferrophosphorus (Fe2P) reacts with pyrite (FeS2) producing iron(II) sulfide and a compound that is 27.87% P and 72.13% S by mass and has a molar mass of 444.56 g/mol. Determine the empirical and molecular formulas of this compound. Empirical Formula: Decimal answers can not be eliminated by rounding up to the nearest whole number.

4 FeS2(s) + 11 O2(g) ® 2 Fe2O3(s) + 8 SO2(g) a) Calculate the mass of Fe2O3 that is produced from the reaction of 75.0 L of O2(g) at 2.33 atm and 150.0oC with an excess of FeS2. b) If the SO2(g) that is generated in (a) is dissolved to form 5.00 L of an aqueous solution, what is the molar concentration of resulting sulfurous acid, H2SO3, solution?

Iron pyrite, FeS2, combines with oxygen from atmosphere to produce iron(III) oxide and sulfur dioxide. If a furnace burns 97.78 g of FeS2, how many grams of SO2 is produced (keep two decimal places)? There’s just one step to solve this.

Question: Part 2 (3 points) FeS2 contains a polyatomic ion. Identify the ions in FeS2, and provide the correct name for the FeS2 compound. Provide the symbol and charge of the iron ion present in Fes2? Fe Provide the symbol and charge of the polyatomic sulfur ion present in FeS2? -1 What is the correct full name of FeS2? Iron (II) disulfide

Question: Ferrophosphorus (Fe2P) reacts with pyrite (FeS2) producing iron(II) sulfide and a compound that is 27.87% P and 72.13% S by mass and has a molar mass of 444.56 g/mol. a) Determine the empirical and molecular formulas of this compound. Empirical Formula: Molecular Formula: b) Write a balanced chemical equation for this reaction.

Question: 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 ram.

Iron pyrite, FeS2, combines with oxygen from atmosphere to produce iron(III) oxide and sulfur dioxide. If a furnace burns 104.98 g of FeS2, how many grams of SO2 is produced? Show transcribed image text

Consider the following reaction at equilibrium. What will happen if some of FeS2 is removed from the reaction? 4 FeS2(s) + 11 O2(g) = 2 Fe2O3(s) + 8 SO2(g) The equilibrium will change in the direction of the reactants. No change in equilibrium is …

Ferrophosphorus (Fe2P) reacts with pyrite (FeS2) producing iron(II) sulfide and a compound that is 27.87% P and 72.13% S by mass and has a molar mass of 444.56 g/mol. Determine the empirical formula of this compound. Express your answer as PxSy Determine the molecular formula of this compound.