@Jup1xcel-es, xve MyLabandMaster CourseHome va MasteringChemisx\"Grona sur deRe

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@Jup1xcel-es, xve MyLabandMaster CourseHome va MasteringChemisx"Grona sur deRe & Secure https://session.masteringchemistry.com/myct/itemView?assignmentProblemID-100596765 ab and Maste ,T- x?E Course Horme Masteringchernis. "Gironi) Sulride Re dn Chapter 7 homework Exercise 7.52 - Enhanced - with Feedback Constants | Periodic Table You may want to reference (Pages 299-306) Section 7.5 while completing this problem. Iron(lI) sulfide reacts with hydrochloric acid according to the Fes(s) +2HCI(aq)-FeClh (aq) +HS(s) Part A A reaction mixture initially contains 0.222 mol FeS and 0.630 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. 0.19 Incorrect: One attempt remaining: Try Again The limiting reactant is the reactant that limits the amount of product in a chemical reaction. Notic makes the least amount of product. The reactant in excess is present in a quantity greater than is reactant. According to the reaction, the amount of HCI consumed is twice the amount of FeS First launch this video. During the video, youl be asked a conceptual question about the example You can watch the video again at any point. Provide Feedback MacBook 4 5 6 2 3

Explanation / Answer

The reaction is Fes(s)+ 2HCl(aq) ---------->FeCl2+ H2S(g)

theoretical molar ratio of FeS: HCl= 1:2

Actual molar ratiio of FeS; HCl =0.22:0.630

dividing by 0.22, the smallest number, the ratio of FeS: HCl becomes 0.222/0.222:0.630/0.222= 1:2.84

so excess is HCl. limiting reactant is FeS. 1 mole of FeS requires 2 mole of HCl.

0.22 moles of FeS requires 2*0.222=0.444 moles of HCl.

So HCl remaining after complete reaction =0.63-0.444= 0.186 moles

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