Iron(II) sulfide reacts with hydrochloric acid according to the reaction:
FeS(s)+2HCl(aq)→FeCl2(s)+H2S(g)
A reaction mixture initially contains 0.214mol FeS and 0.636mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?

Question

Iron(II) sulfide reacts with hydrochloric acid according to the reaction:
FeS(s)+2HCl(aq)→FeCl2(s)+H2S(g)
A reaction mixture initially contains 0.214mol FeS and 0.636mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?

anonymous · Answer

This can be a toughie. Start with the limiting reactant stoichometery....