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7 March, 21:20

After substantial heating, 6.25 g of iron produced 18.00 g of a compound with chlorine. The empirical formula is:

a. FeCl3

b. Fe3Cl

c. Fe2Cl3

d. FeCl2

e. Fe2Cl

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Answers (1)
  1. 8 March, 00:11
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    Option A. FeCl3

    Explanation:

    The following data were obtained from the question:

    Mass of iron (Fe) = 6.25g

    Mass of the compound formed = 18g

    From the question, we were told that the compound formed contains chlorine. Therefore the mass of chlorine is obtained as follow

    Mass of chlorine (Cl) = Mass of compound formed - Mass of iron.

    Mass of chlorine (Cl) = 18 - 6.25

    Mass of chlorine (Cl) = 11.75g

    The compound therefore contains:

    Iron (Fe) = 6.25g

    Chlorine (Cl) = 11.75g

    The empirical formula for the compound can be obtained by doing the following:

    Step 1:

    Divide by their molar mass

    Fe = 6.25/56 = 0.112

    Cl = 11.75/35.5 = 0.331

    Step 2:

    Divide by the smallest

    Fe = 0.112/0.112 = 1

    Cl = 0.331/0.112 = 3

    The empirical formula for the compound is FeCl3
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