Final answer:
The reaction between iron(II) sulfide and hydrochloric acid is explained using a balanced chemical equation. The ratio of reactants is determined based on the coefficients in the equation. The excess of HCl in the reaction is also calculated.
Step-by-step explanation:
The subject of this question is Chemistry. The question asks about the reaction between iron(II) sulfide and hydrochloric acid. The balanced chemical equation for this reaction is:
FeS(s) + 2HCl(aq) → FeCl2(aq) + H2S(g)
In this reaction, 0.226 mol of FeS and 0.642 mol of HCl are present in the reaction mixture. By comparing the coefficients in the balanced equation, we can determine that the ratio of FeS to HCl is 1:2. Therefore, 0.226 mol of FeS will react with 2 * 0.226 mol = 0.452 mol of HCl. The remaining 0.642 mol - 0.452 mol = 0.19 mol of HCl will be in excess.
The student's question pertains to a chemical reaction between iron(II) sulfide (FeS) and hydrochloric acid (HCl), producing iron(II) chloride (FeCl2) and hydrogen sulfide gas (H2S). Given initial amounts of 0.226 mol FeS and 0.642 mol HCl, it is important to determine which reactant is the limiting reagent that will determine the extent of the reaction and the amounts of products formed.
The balanced chemical equation for the reaction is: FeS(s) + 2HCl(aq) → FeCl2(aq) + H2S(g). This shows that each mole of FeS requires two moles of HCl to react completely. Since the amount of HCl present is more than double the amount of FeS, FeS is the limiting reagent and will determine the final quantities of the products. Using stoichiometry, one can calculate the amount of FeCl2 and H2S that will be formed.