I only have about 45 minutes to figure this out:
Have posted it before and the response I got did not come to the right answer

Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) right arrow FeCl2(s) + H2S(g) A reaction mixture initially contains 0.175 mol FeS and 0.481 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?

Question

I only have about 45 minutes to figure this out:
Have posted it before and the response I got did not come to the right answer

Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) right arrow FeCl2(s) + H2S(g) A reaction mixture initially contains 0.175 mol FeS and 0.481 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?