Ask Question
27 May, 08:33

A 43.56 gram sample of iron is heated in the presence of excess sulfur. A metal sulfide is formed with a mass of 81.08 g. Determine the empirical formula of the metal sulfide.

+1
Answers (1)
  1. 27 May, 11:19
    0
    Fe2S3

    Explanation:

    Data obtained from the question include:

    Mass of Fe = 43.56g

    Mass of metal sulfide = 81.08g

    Next we shall determine the mass of sulphur, S in the compound. This is illustrated below:

    Mass of S = Mass of metal sulfide - mass of Fe

    Mass of S = 81.08 - 43.56 = 37.52g

    The empirical formula for the metal sulfide can be obtain as follow:

    Fe = 43.56g

    S = 37.52g

    Divide by their molar mass

    Fe = 43.56/56 = 0.7779

    S = 37.52/32 = 1.1725

    Divide by the smallest

    Fe = 0.7779/0.7779 = 1

    S = 1.1725/0.7779 = 1.5

    Multiply through by 2 to express in whole number

    Fe = 1 x 2 = 2

    S = 1.5 x 2 = 3

    Therefore, the empirical formula for the metal sulfide is Fe2S3
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “A 43.56 gram sample of iron is heated in the presence of excess sulfur. A metal sulfide is formed with a mass of 81.08 g. Determine the ...” in 📘 Chemistry if you're in doubt about the correctness of the answers or there's no answer, then try to use the smart search and find answers to the similar questions.
Search for Other Answers