What is the empirical formula of a compound that has a molar mass of 42 grams and an empirical formula of CH2?Group of answer choicesCH2C2H4C4H12C3H6

The empirical formula of a compound is the simplest, most reduced ratio of elements in a compound. In this case, the empirical formula is given as CH2.

The molar mass of CH2 can be calculated by adding the molar mass of Carbon (C) and twice the molar mass of Hydrogen (H). The molar mass of Carbon is approximately 12.01 g/mol and the molar mass of Hydrogen is approximately 1.01 g/mol.

So, the molar mass of CH2 = 12.01 g/mol (for C) + 2(1.01 g/mol) (for H) = 14.03 g/mol

The given molar mass of the compound is 42 g/mol.

To find the ratio of the molar mass of the compound to the molar mass of the empirical formula, we divide the molar mass of the compound by the molar mass of the empirical formula:

42 g/mol ÷ 14.03 g/mol = 3

This means that the molecular formula of the compound is three times the empirical formula. Therefore, the molecular formula of the compound is C3H6.