3uckyidn
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What is the empirical formula of [tex]$C _8 H _{16} O _8$[/tex]?

A. [tex]$CH _2 O _2$[/tex]
B. [tex][tex]$C _2 H _4 O _2$[/tex][/tex]
C. [tex]$CH _2 O$[/tex]
D. CHO

Sagot :

GinnyAnsweridn
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]
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