Question

Part A

A sample of a compound is decomposed in the laboratory and produces 330 g carbon, 69.5 g hydrogen, and 440.4 g oxygen. Calculate the empirical formula of the compound.
Express your answer as an empirical formula.

Answer 1

I got this. I hope this helps. :/

Answer 2

C₂H₅O₂

Step-by-step explanation:

The empirical formula, is the reduced formula of a compound, with the elements followed by its smallest possible number of moles.

First, let's calculated the number of moles of each element. The molar masses are:

C = 12 g/mol, H = 1 g/mol, O = 16 g/mol

The number of moles is the mass divided by molar mass, so :

nC = 330/12 = 27.5

nH = 69.5/1 = 69.5

nO = 440.4/16 = 27.5

To have the empirical formula, let's divide all the number of moles for the smallest: 27.5

nC = 27.5/27.5 = 1

nH = 69.5/27.5 = 2.5

nO = 27.5/27.5 = 1

The empirical formula can't have fractional numbers, so let's multiply all the numbers for 2

nC = 2

nH = 5

nO = 2

The empirical formula is

C₂H₅O₂