For this question we will find the empirical formula and the molecular formula for a compound made of 39.7458% of C, 2.77956% of H, 13.4050% of Mg, and 44.0697% of Br. The mass we are calculating will be 181.33g/mol. The first thing we need to do is to find out how many grams of each element we actually have:
181.33g/mol = 100%
x grams = 39.7458%
x = 72.07 grams of C
181.33 = 100%
x grams = 2.77956%
x = 5.04 grams of H
181.33 = 100%
x grams = 13.4050%
x = 24.307 grams of Mg
181.33 = 100%
x grams = 44.0697%
x = 79.91 grams of Br
Now we have the mass for each element, we need to find the number of moles that each element has based on their masses and the molar mass of each one:
Carbon = 12g/mol
H = 1g/mol
Mg = 24.305g/mol
Br = 79.9g/mol
For Carbon:
12g = 1 mol
72.07g = x moles
x = 6 moles of C
For Hydrogen:
1g = 1 mol
5.04g = x moles
x = 5 moles of H
For Magnesium:
24.305g = 1 mol
24.307g = x moles
x = 1 mol of Mg
For Bromide:
79.90g = 1 mol
79.91g = x moles
x = 1 mol of Br
The molecular formula for this compound will be C6H5MgBr, this is Phenylmagnesium bromide, this will also be its empirical formula, since there is no way we can divide the numbers and make an empirical formula.