MISSED THIS? Watch KCV: Limiting Reactant, Theoretical Yield, and Percent Yield, IWE: Limiting Reactant and Theoretical Yield; Read Section 4.4. You can click on the Review link to access the section in your eText. Iron(II) sulfide reacts with hydrochloric acid according to the reaction FeS (s) + 2HCl(aq)→FeCl₂ (aq) + H₂S(s) A reaction mixture initially contains 0.212 mol FeS and 0.636 mol HCl. Part A 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. IVE ΑΣΦ n = Submit Request Answer ? mol

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MISSED THIS? Watch KCV: Limiting Reactant, Theoretical Yield,
and Percent Yield, IWE: Limiting Reactant and Theoretical
Yield; Read Section 4.4. You can click on the Review link to
access the section in your eText.
Iron(II) sulfide reacts with hydrochloric acid according to the
reaction
FeS (s) + 2HCl(aq)→FeCl₂ (aq) + H₂S(s)
A reaction mixture initially contains 0.212 mol FeS and 0.636
mol HCl.
Part A
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.
n =
Submit
V
ΑΣΦ
Request Answer
?
mol
Transcribed Image Text:MISSED THIS? Watch KCV: Limiting Reactant, Theoretical Yield, and Percent Yield, IWE: Limiting Reactant and Theoretical Yield; Read Section 4.4. You can click on the Review link to access the section in your eText. Iron(II) sulfide reacts with hydrochloric acid according to the reaction FeS (s) + 2HCl(aq)→FeCl₂ (aq) + H₂S(s) A reaction mixture initially contains 0.212 mol FeS and 0.636 mol HCl. Part A 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. n = Submit V ΑΣΦ Request Answer ? mol
Expert Solution
Step 1

Iron(II) sulfide reacts with hydrochloric acid to form iron(II) chloride and hydrogen sulfide. The equation for the balanced chemical reaction is as follows:

FeSs + 2HClaq   FeCl2aq + H2Ss

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