To determine the empirical formula of a given compound, we need to simplify the molecular formula to its simplest whole number ratio of each element present in the compound.
Given the molecular formula: [tex]\( C_8 H_{16} O_8 \)[/tex]
First, we identify the subscripts of each element in the molecular formula:
- Carbon (C) subscript: 8
- Hydrogen (H) subscript: 16
- Oxygen (O) subscript: 8
Next, we find the greatest common divisor (GCD) of these subscripts to simplify them. The GCD of 8, 16, and 8 is 8.
Now, we divide each subscript by the GCD to get the simplest form:
- Carbon: [tex]\( \frac{8}{8} = 1 \)[/tex]
- Hydrogen: [tex]\( \frac{16}{8} = 2 \)[/tex]
- Oxygen: [tex]\( \frac{8}{8} = 1 \)[/tex]
So the simplified subscripts are:
- C: 1
- H: 2
- O: 1
Thus, the empirical formula of [tex]\( C_8 H_{16} O_8 \)[/tex] is:
[tex]\[ CH_2O \][/tex]
The other options are:
- [tex]\( CH_2O_2 \)[/tex]
- [tex]\( C_2H_4O_2 \)[/tex]
- [tex]\( CHO \)[/tex]
However, the correct empirical formula based on the simplest whole number ratio is:
[tex]\[ CH_2O \][/tex]
