Question

Iron(II) sulfide reacts with hydrochloric acid according to the reaction FeS(s) + 2HCl(aq) → FeCl₂(aq) + H₂S(g). A reaction mixture initially contains 0.232 mol FeS and 0.630 mol HCl.

Answer 1

The reaction between iron(II) sulfide and hydrochloric acid involves stoichiometry and limiting reactants. Given 0.232 mol FeS and 0.630 mol HCl, HCl is the limiting reactant. The stoichiometry of the reaction will determine the amounts of products and leftover reactants.

Step-by-step explanation:

The reaction between iron(II) sulfide (FeS) and hydrochloric acid (HCl) is a chemical process that can be classified as a single replacement reaction and also as a redox reaction since there is a transfer of electrons with the sulfur being oxidized. To determine the limiting reactant and the amounts of products formed, we apply stoichiometry: we need 2 moles of HCl for every 1 mole of FeS according to the reaction equation FeS(s) + 2HCl(aq) → FeCl₂(aq) + H₂S(g). Given the initial moles of FeS and HCl, we can calculate how much of each reactant will be consumed and how much of each product will be produced.

Here, 0.232 mol FeS reacts with 0.630 mol HCl. Since the molar ratio is 1:2 and we have only 0.630 mol HCl available, HCl is the limiting reactant. By dividing the moles of HCl available by 2, we get 0.315 mol, which is greater than the 0.232 mol of FeS, indicating that all of the FeS can react, and there will be excess HCl left.