Question

An alcohol is 68.84 % C and 4.962 % H by mass. The rest is oxygen. What is the empirical formula of the alcohol? Enter the elements in the order C, H, and then O.

Answer 1

The empirical formula is C₇H₆O₂.

Assume that you have 100 g of the compound.

Then you have 68.84 g C and 4.962 g H.

Mass of O = (100 – 68.84 – 4.962) g = 26.20 g O.

Now, we must convert these masses to moles and find their ratios.

From here on, I like to summarize the calculations in a table.

Element     Mass/g    Moles    Ratio     ×2   Integers  

     C           68.84      5.732    3.501  7.001       7

     H            4.962    4.923    3.006  6.012      6

     O          26.20      1.638     1          2             2

The empirical formula is C₇H₆O₂.

Answer 2

The empirical formula is C₇H₆O₂ which contains 7 atoms of carbon, six atoms of hydrogen, and two-atoms of oxygen.

What is an empirical formula?

A chemical formula showing the simplest ratio of elements in a compound rather than the total number of atoms in the molecule $CH_2O$ is the empirical formula for glucose.

Assume that you have 100 g of the compound.

Given data:

Mass of carbon = 68.84 g

Mass of hydrogen = 4.962 g H.

Mass of oxygen = (100 – 68.84 – 4.962) g = 26.20 g.

Now, we must convert these masses to moles and find their ratios.

Element     Mass/g   Moles   Ratio     ×2   Integers  

    C           68.84      5.732    3.501  7.001       7

    H           4.962    4.923    3.006  6.012      6

   O          26.20      1.638     1          2             2

Hence, the empirical formula is C₇H₆O₂.

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