Chemistry, 26.06.2019 11:00 bermudezs732

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-.

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Answer from: elenadelfosse

The empirical formula of the compound is Fe_1S_1O_4

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= $\frac{36.76 g}{55.84 g/mol}=0.658 mol$

Moles of sulfur= $\frac{21.11 g}{32.06 g/mol}=0.658 mol$

Moles of oxygen= $\frac{42.13 g}{16 g/mol}=2.633 mol$

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 = $\frac{0.658 mol}{0.658 mol}=1$

For sulfur element = $\frac{0.658 mol}{0.658 mol}=1$

For oxygen element = $\frac{2.633 mol}{0.658 mol}=4.001\approx 4$

So, the empirical formula of the compound is Fe_1S_1O_4

Answer from: kitttimothy55

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:

$Fe: \dfrac{36.76\:\diagup\!\!\!\!\!g}{55.84\:\diagup\!\!\!\!\!g/mol} \approx 0.658\:mol$

$S: \dfrac{21.11\:\diagup\!\!\!\!\!g}{32.06\:\diagup\!\!\!\!\!g/mol} \approx 0.658\:mol$

$O: \dfrac{42.13\:\diagup\!\!\!\!\!g}{16\:\diagup\!\!\!\!\!g/mol} \approx 2.633\:mol$

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:

$Fe: \dfrac{0.658}{0.658}\to\:\:\boxed{Fe = 1}$

$S: \dfrac{0.658}{0.658}\to\:\:\boxed{S = 1}$

$O: \dfrac{2.633}{0.658}\to\:\:\boxed{O \approx 4}$

Thus, the minimum or empirical formula found for the compound will be:

$\boxed{\boxed{Fe_1S_1O_4\:\:\:or\:\:\:FeSO_4}}\Longleftarrow(Empirical\:Formula)\end{array}}\qquad\checkmark$

FeSO4 - Iron (II) Sulfate

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I Hope this helps, greetings ... Dexteright02! =)

Answer from: Quest

answer: option (b) is the correct answer.

explanation:

a covalent bond is formed by sharing of electrons. whereas polarity arises due to difference in electronegativity of two atoms.

therefore, more is the electronegativity of an atom which combines with the titanium, more readily it will induce a partial positive and negative charge.

thus, out of the given options fluorine is most electronegative and has an incomplete octet. therefore, it will readily combine with titanium to share the electrons and complete its octet.

Answer from: Quest

You use the atomic number to find out how many protons and neutrons there are in the atom. you use the atomic mass to find out how many protons and electrons there are in the atom.