Iron(II) sulfide reacts with hydrochloric acid according to the reaction:
FeS(s)+2HCl(aq)→FeCl2(s)+H2S(g)
A reaction mixture initially contains 0.200 mol FeS and 0.674 mol HCl.
The question is:
Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?
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2017-03-14 10:25 pm
回答 (1)
2017-03-14 10:47 pm
✔ 最佳答案
FeS(s) + 2HCl(aq) → FeCl₂(s) + H₂S(g)Mole ratio FeS : HCl = 1 : 2
If 0.200 mol FeS completely reacts :
No. of moles of HCl needed = (0.200 mol) × 2 = 0.400 mol < 0.674 mol
Hence, HCl is in excess.
No. of moles of HCl left = (0.674 - 0.400) mol = 0.274 mol
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