Find the empirical and molecular formula for a molar mass of 60.10g/mol; 39.97% carbon 13.41% hydrogen: 46.62% nitrogen

Assuming we have 100g, this means that

39.97g Carbon * 1 mol / 12 g = 3.33 mol Carbon
13.41g Hydrogen * 1 mol/1 g = 13.41 mol Hydrogen
46.62g Nitrogen * 1 mol / 14 g = 3.33 mol Nitrogen
Dividing everything by 3.33, we get

1 mol Carbon, 4.03 mol Hydrogen, 1 mol Nitrogen.

Empirical formula is CH4N

The mass of the empirical formula is
12 + 4 + 14 = 30

Since the molar mass is double, we multiply all our subscripts

The molecular formula is C2H8N2

The answers to this question are an empirical formula of CH4N and a molecular formula of C2H8N2 .

Sorry i dont understand the question can you rephase it?