Lesson 13 Question 8 Part A At high temperatures, sulfur combines with iron to f

Question

Lesson 13 Question 8 Part A At high temperatures, sulfur combines with iron to form the brown-black iron(lI) sulfide Fe(s) + S (l) FeS (s) n one experiment, 7.62 g of Fe are allowed to react with 8.67 g of S. What is the limiting reagent, what is the mass of FeS formed, and how much excess reagent is left, respectively? Express your answer numerically to three significant figures. O Fe, 23.8 g FeS, 1.05 gs Fe, 12.0 g Fes, 4.29 g S S, 23.8 g FeS, 1.05 g Fe OS, 238 g FeS, 1.05g Fe S, 12.0 g FeS, 1.05 g Fe S, 12.0 g Fes, 1.05 g Fe Submit Hints My Answers Give Up Review Part

Explanation / Answer

Fe (s) + S (l) FeS (s)

No of mole of Fe = 7.62/55.845 = 0.1364 mol

No of mol of S = 8.67/32 = 0.271 mol

from equation

1 mol Fe = 1mol S

limiting reagent is Fe

No of mol of Fes produced = 0.1364 mol

mass of Fes = 0.1364*87.910 = 11.99 grams

excess reagent is S

mass of excess reagent left = (0.271-0.1364)*32 = 4.31 grams

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