A compound is found to contain 39.99 % carbon, 6.727 % hydrogen, and 53.28 % oxygen by weight. To answer the questions, enter the elements in the order presented above. 1. What is the empirical formula for this compound

CH₂O

Explanation:

The empirical formula is the simplest whole-number ratio of atoms in a compound.

The ratio of atoms is the same as the ratio of moles.

So, our job is to calculate the molar ratio of C:H:O.

Assume 100 g of the compound.

1. Calculate the mass of each element.

Then we have 39.99 g C, 6.727 g H, and 53.28 g O.

2. Calculate the moles of each element

3. Calculate the molar ratio of the elements

Divide each number by the smallest number of moles

C:H:O = 3.330:6.674:3.330 = 1:2.004:1.000 ≈ 1:2:1

4. Write the empirical formula

EF = CH₂O

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