If a molecule with an empirical formula of CH_(2)O has a molar mass of 60, what is the molecular formula? C_(2)H_(4)O C_(4)H_(8)O_(4) C_(2)H_(4)O_(2) CH_(4)O_(2)

To determine the molecular formula of a molecule with an empirical formula of and a molar mass of 60, we need to find the ratio of the molar mass of the empirical formula to the given molar mass.The molar mass of the empirical formula is calculated as follows:- Carbon (C): 12.01 g/mol- Hydrogen (H): 1.01 g/mol (since there are 2 hydrogen atoms, multiply by 2)- Oxygen (O): 16.00 g/molSo, the molar mass of is: Next, we divide the given molar mass (60 g/mol) by the molar mass of the empirical formula (30.03 g/mol): This indicates that the molecular formula is twice the empirical formula. Therefore, we multiply each subscript in the empirical formula by 2: Thus, the molecular formula is: