determine the molecular mass of a compound that contains 42.87% carbon, 3.598% hydrogen, 28.55% oxygen and 25.00% hydrogen if the molar mass is 168 g/mol

Answer 1

This is an empirical formula problem.

Pretend percentages are grams, and convert to moles.

C: 42.87/12.01=3.569 mol

H: 3.598/1.008=3.5694 mol

O: 28.55/16.00=1.7843 mol

Now i'm realizing there is a typo because you put hydrogen twice. I assume one is supposed to be nitrogen, but until then, this is impossible to solve.