Question

A compound is found to contain 50. 05% sulfur and 49. 95% oxygen by mass. What is the empirical formula for this compound? SO S2O SO2 What is the empirical mass of that compound? Answer using four significant figures. G.

Answer 1

The empirical formula for the given compound has been $\rm SO_2$. Thus, option C is correct.

The empirical formula has been the whole unit ratio of the elements in the formula unit.

Computation for the Empirical formula

The given mass of Sulfur has been, 50.05 g

The given mass of oxygen has been 49.95 g.

The moles of elements in the sample has been given by:

$\rm Moles=\dfrac{Mass}{Molar\;mass}$

• Moles of Sulfur:

$\rm Moles\;S=\dfrac{50.05}{32}\\ Moles\;S=1.56\;mol$

The moles of sulfur in the unit has been 1.56 mol.

• Moles of Oxygen:

$\rm Moles\;O=\dfrac{49.95}{16} \\ Moles\;O=3.12\;mol$

The moles of oxygen in the unit has been 3.12 mol.

The empirical formula unit has been given as:

$\rm S_{1.56}O_{3.12}=SO_2$

Thus, the empirical formula for the given compound has been $\rm SO_2$. Thus, option C is correct.

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