Question

A strip of iron weighing 0.95g is placed in the flask and allowed to react with the sulfur. If the weight of the new compound is 77g, determine:

      (Fe = 55.85g/mol and S = 32.06g/mol)

            a. The mass of sulfur reacted = _______________

            b. The mass percent Fe and S based on the experiment

  

                        %Fe =

                        %S =

            c. The empirical formula of the compound.

Answer 1

S Fes Reaction: Fe + (Iron) (sulfurs Molar mass of fes (Iron sulfides 55.35 g Imol . 0.95 g fe 0.95 g. Fe 55:85 g. null 0,olt mol Fe 1 mol Fe reacts with. 1 mot S 0.017 mol Fe reacts with 0.017 mois Molar mass of s= 32.06 orolt mol. s 0,017 molx 32.06 gomoin S S. a of sulfur reacted = MOSS 0.5950 The mass of 0.545 g Molar mess of Fes If g 12 s - (55.85+ 32.00) gimon 87.91 Ef g Fes Fes c.0.876 noi 87.91 Fes. 1 mol Fes contains 1 mol Fe. o. Sto go! Fes contarys 8.876noy Fe TE fes ma gonor g . g g g g Fe 8.7.91 Fes contains 55:55 IF Fes contains 55.55 X FT 87.91 = 49.92 i100 Fes contains a 49.92X.100 FF CS Scanned with CamScanner = 64.83 Fe g Fe of Fe 8 g

1Mass percentage of Fe = 64.83 . Again, Si.al 32.06 Fes contains soon j S , FI Fes contains g. S ot 32.06 8.77 8791 28, 08 S ot Fes contains S 28.08 x 100 FT 36.47 g que LU s Mass i 6 Now 64.83 g percentage of $ =: 36.47%. 64.83 g 55.85 g.mor gs Fe Fe= I 1.16 mol Fe 36.47 36.47 g S 32.06 giment . 1:1.4 mol S Let the emperical formulate of the compound will be feasy Now for we will divide both moles by smallest number of moles between these two. calculating x y OS 1 1.16 1.14 1:19 y 2 1:14 The emperical formulai of the Compound will be Fest Fes CS Scanned with CamScanner