Final answer:
The molecular formula is found to be twice the empirical formula based on the given molecular weight, leading to the answer being B) C2H8N2.
Step-by-step explanation:
The molecular formula of a compound with the empirical formula CH4N and a molecular weight of 60.0g can be found by determining the mass of the empirical formula and then establishing how many times that empirical formula mass divides into the molecular weight. The mass of CH4N is 12.01 (C) + 4(1.01) (H) + 14.01 (N) = 30.05g/mol. Since the molecular weight is twice that of the empirical formula mass (60.0 / 30.05 ≈ 2), the molecular formula is a multiple of the empirical formula. Therefore, the correct answer is B) C2H8N2.