This problem is providing us with the percent composition of a compound containing sodium, bromine and oxygen. Thus, the empirical formula is required and found to be NaBrO₃.
In chemistry, empirical formulas are used in order to figure out the minimum whole-number representation of a molecular formula, which contains the actual number of atoms.
Thus, we start determining it by assuming the given percentages as masses and calculating the moles with the atomic mass of the involved elements:
[tex]n_{Na}=\frac{15.24}{22.99}=0.700 \\\\n_{Br}=\frac{52.95}{79.90} =0.663\\\\n_O=\frac{31.81}{16.00}=1.99[/tex]
Next, we divide by the 0.633 as the smallest number of moles in order to determine their subscripts in the chemical formula:
[tex]Na:\frac{0.700}{0.663}=1\\ \\Br:\frac{0.663}{0.663}=1\\ \\O=\frac{1.99}{0.663} =3[/tex]
Hence, the empirical formula turns out to be NaBrO₃.
Learn more about percent composition: brainly.com/question/12247957
