Question

select the correct answer from each drop - down menu.
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
cl
.
use the periodic table to help you find the molar masses.

Explanation:

Step1: Find moles of Fe

Molar mass of Fe is \(55.85\space g/mol\). Moles of Fe = \(\frac{143\space g}{55.85\space g/mol} \approx 2.56\space mol\)

Step2: Find moles of Cl

Molar mass of Cl is \(35.45\space g/mol\). Moles of Cl = \(\frac{273\space g}{35.45\space g/mol} \approx 7.70\space mol\)

Step3: Find mole ratio

Divide moles by the smallest (2.56):
Fe: \(\frac{2.56}{2.56} = 1\)
Cl: \(\frac{7.70}{2.56} \approx 3\)

Answer:

The empirical formula is \(FeCl_3\) (so the subscripts are 1 for Fe and 3 for Cl).