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A sample of a compound weighing 416 grams decomposes into 143 grams of iron and 273 grams of chlorine. The
percent composition of these products is
iron and chlorine. Using these values, we can
determine that the empirical formula of the compound is Fe CI
Use the periodic table to help you find the molar masses.

A sample of a compound weighing 416 grams decomposes into 143 grams of iron and 273 grams of chlorine The percent composition of these products is iron and chl class=

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Eduard22sly

1. The percentage composition of iron in the compound is 34.4%

2. The percentage composition of chlorine in the compound is 65.6%

3. The empirical formula of the compound is FeCl₃

1. How to determine the percentage of iron

  • Mass of compound = 416 g
  • Mass of iron (Fe) = 143 g
  • Percentage of iron (Fe) =?

Percentage of Fe = (mass of Fe / mass of compound) × 100

Percentage of Fe = (143 / 416) × 100

Percentage of Fe = 34.4%

2. How to determine the percentage of chlorine

  • Percentage of Fe = 34.4%
  • Total percentage = 100%
  • Percentage of chlorine (Cl) =?

Percentage of Cl = 100 – 34.4

Percentage of Cl = 65.6%

3. How to determine the empirical formula

  • Fe = 34.4%
  • Cl = 65.6%
  • Empirical formula =?

Divide by their molar mass

Fe = 34.4 / 56 = 0.614

Cl = 65.6 / 35.5 = 1.848

Divide by the smallest

Fe = 0.614 / 0.614 = 1

Cl = 1.848 / 0.614 = 3

Thus, the empirical formula of the compound is FeCl₃

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