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Vesnalui [34]
2 years ago
5

A compound is found to contain 50. 05% sulfur and 49. 95% oxygen by mass. What is the empirical formula for this compound? SO S2

O SO2 What is the empirical mass of that compound? Answer using four significant figures. G.
Chemistry
1 answer:
jekas [21]2 years ago
8 0

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.

<h3>Computation for the Empirical formula</h3>

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}\\&#10; 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} \\&#10;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.

Learn more about empirical formula, here:

brainly.com/question/11588623

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