Verified answer

I actually worked it out, but the final molecular formula was not in a whole number ratio. Therefore, I believe that the variables you provided were not the accurate ones.

Basically, first you have to find the mole ratio by dividing the molar mass by the mass for each element, ie. (mass of carbon/ molar mass) and (mass of hydrogen/ molar mass) Then, you have to divide both ratios (of both elements) by the smallest mole ratio (that could be either carbon's or hydrogen's). That should give you the empirical formula.

Using the empirical formula, you can find the empirical mass, and you use the periodic table for this.

Then use the following formula to find the common ratio between the molecular formula and the empirical formula:

n= (empirical mass/ molecular mass).

Then multiply the empirical formula by the result, n. This will give you the molecular formula.

i think there's a prob in the question...

this is the formula in getting the MF:

MF = EF[ MW/EW]