A compound has an empirical formula of C2H4O and a molar mass of 88 grams per mole. What is the molecular formula of this compound?

 Oct 17, 2017


A compound's empirical formula tells you the smallest whole number ratio that exists between the elements that make up a compound.

In your case, the unknown compound has an empirical formula of C2H4O, which means that it contains carbon, C, hydrogen, H, and oxygen, O, in a 2:4:1 ratio.

In other words, one mole of this compound will contain carbon, hydrogen, and oxygen in a 2:4:1 mole ratio.

All you have to do now is determine the mass of the empirical formula and compare it with the molar mass of the compound. You will have

2×12.011 g mol−1+4×1.00794 g mol−1+1×15.9994 g mol−1=44.053 g mol−1

The molar mass of the compound essentially tells you the mass of one mole of the compound. This means that you will have

44.053g mol−1×n=88g mol−1

Rearrange to get

n=88 / 44.053=1.9976≈2

Therefore, the molecular formula of the compound, which tells you the exact number of atoms of each element present in one molecule of the compound, will be:

(C2H4O)2 =C4H8O2

 Oct 17, 2017
edited by Guest  Oct 17, 2017


You could have posted this link




It’s neater than your slop copy you plagiarized and posted here. frown

 Oct 17, 2017

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