Respuesta :
Answer: The empirical formula of the compound is [tex]Fe_1S_1O_4[/tex]
Explanation:
Empirical formula is defined formula which is simplest integer ratio of number of atoms of different elements present in the compound.
Percentage of iron in a compound = 36.76 %
Percentage of sulfur in a compound = 21.11 %
Percentage of oxygen in a compound = 42.13 %
Consider in 100 g of the compound:
Mass of iron in 100 g of compound = 36.76 g
Mass of iron in 100 g of compound = 21.11 g
Mass of iron in 100 g of compound = 42.13 g
Now calculate the number of moles each element:
Moles of iron=[tex]\frac{36.76 g}{55.84 g/mol}=0.658 mol[/tex]
Moles of sulfur=[tex]\frac{21.11 g}{32.06 g/mol}=0.658 mol[/tex]
Moles of oxygen=[tex]\frac{42.13 g}{16 g/mol}=2.633 mol[/tex]
Divide the moles of each element by the smallest number of moles to calculated the ratio of the elements to each other
For Iron element = [tex]\frac{0.658 mol}{0.658 mol}=1[/tex]
For sulfur element = [tex]\frac{0.658 mol}{0.658 mol}=1[/tex]
For oxygen element = [tex]\frac{2.633 mol}{0.658 mol}=4.001\approx 4[/tex]
So, the empirical formula of the compound is [tex]Fe_1S_1O_4[/tex]
Hello!
What is the empirical formula? A compound is used to treat iron deficiency in people. It contains 36.76% iron, 21.11% sulfur, and 42.13% oxygen. The empirical formula is Fe-S-O-.
data:
Iron (Fe) ≈ 55.84 a.m.u (g/mol)
Sulfur (S) ≈ 32.06 a.m.u (g/mol)
Oxygen (O) ≈ 16 a.m.u (g/mol)
We use the amount in grams (mass ratio) based on the composition of the elements, see: (in 100g solution)
Fe: 36.76 % = 36.76 g
S: 21.11 % = 21.11 g
O: 42.13 % = 42.13 g
The values (in g) will be converted into quantity of substance (number of mols), dividing by molecular weight (g / mol) each of the values, we will see:
[tex]Fe: \dfrac{36.76\:\diagup\!\!\!\!\!g}{55.84\:\diagup\!\!\!\!\!g/mol} \approx 0.658\:mol[/tex]
[tex]S: \dfrac{21.11\:\diagup\!\!\!\!\!g}{32.06\:\diagup\!\!\!\!\!g/mol} \approx 0.658\:mol[/tex]
[tex]O: \dfrac{42.13\:\diagup\!\!\!\!\!g}{16\:\diagup\!\!\!\!\!g/mol} \approx 2.633\:mol[/tex]
We realize that the values found above are not integers, so we divide these values by the smallest of them, so that the proportion does not change, let us see:
[tex]Fe: \dfrac{0.658}{0.658}\to\:\:\boxed{Fe = 1}[/tex]
[tex]S: \dfrac{0.658}{0.658}\to\:\:\boxed{S = 1}[/tex]
[tex]O: \dfrac{2.633}{0.658}\to\:\:\boxed{O \approx 4}[/tex]
Thus, the minimum or empirical formula found for the compound will be:
[tex]\boxed{\boxed{Fe_1S_1O_4\:\:\:or\:\:\:FeSO_4}}\Longleftarrow(Empirical\:Formula)\end{array}}\qquad\checkmark[/tex]
Answer:
FeSO4 - Iron (II) Sulfate
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I Hope this helps, greetings ... Dexteright02! =)
