Iron(II) sulfide reacts with hydrochloric acid according to the reactionFeS(s)+2HCl(aq)→FeCl2(aq)+H2S(s)A reaction mixture initially contains 0.228 mol FeS and 0.664 mol HCl.Once the reaction has reached completion, what amount (in moles) of the excess reactant is left?Express the answer in moles to three significant figures.

Question
Asked Oct 3, 2019

Iron(II) sulfide reacts with hydrochloric acid according to the reaction

FeS(s)+2HCl(aq)→FeCl2(aq)+H2S(s)

A reaction mixture initially contains 0.228 mol FeS and 0.664 mol HCl.

Once the reaction has reached completion, what amount (in moles) of the excess reactant is left?
Express the answer in moles to three significant figures.
 
 
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Expert Answer

Step 1

The values are given as follows:

iniially moles of FeS = 0.228 mol
initially moles of HCl 0.664 mol
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iniially moles of FeS = 0.228 mol initially moles of HCl 0.664 mol

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Step 2

The balanced chemical equation is given as follows:

Fes(s)+2HC1(aq)> FeCl, (aq) +H,Ss)
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Fes(s)+2HC1(aq)> FeCl, (aq) +H,Ss)

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Step 3

Since, the ratio between FeS and HCl indicates 1:2. Therefore,...

moles of HCl 0.228 mol FeS x 2 mol HCI
1 mol FeS
0.456 mol HCI
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moles of HCl 0.228 mol FeS x 2 mol HCI 1 mol FeS 0.456 mol HCI

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