In every 100g of that compund there is 50.84 g of C, 8.53 g H and (100-59.37) g = 40.63 g of O.
Step 1: Convert each element's mass in moles. To do that we need to divide each element's mass by their respective molar mass.
For Carbon.
[tex]C = \frac{50.84}{12} = 4.24 mol [/tex]
For Hydrogen.
[tex]H = \frac{8.53}{1} = 8.53 mol [/tex]
For Oxygen.
[tex]O = \frac{40.63}{16} = 2.54 mol [/tex]
Step 2: Divide each of the numbers by the smallest number.
For Carbon.
[tex]C = \frac{4.24}{2.54} = 1.7 [/tex]
For Hydrogen.
[tex]H = \frac{8.53}{2.54} = 3.36 [/tex]
For Oxygen.
[tex]O = \frac{2.54}{2.54} = 1 [/tex]
Step 3: So the empirical formula will be.
[tex] C_{1.7} H_{3.36} O_1 [/tex]
But using decimal will be messy. So we multiply the numbers by 3. The right empirical formula will be.
[tex] C_{5} H_{10} O_3 [/tex]
The empirical formula of an organic compound that contains 50.84% C, 8.53% H, and the rest oxygen is C₅H₁₀O₃.
First, we have to determine the mass percentage of oxygen, knowing that C, H and O amount to the 100% of the compound.
[tex]C + H + O = 100\%\\O = 100\% - C - H\\O = 100\% - 50.84\% - 8.53\% = 40.63\%[/tex]
Then, we divide each mass percentage by the atomic mass of the element.
[tex]C: 50.84/12.01 = 4.23\\H: 8.53/1.01 = 8.45\\O: 40.63/16.00 = 2.54[/tex]
Afterwards, we divide all the numbers by the smallest one, i.e. 2.54.
[tex]C: 4.23/2.54 = 1.66\\H: 8.45/2.54 = 3.33\\O: 2.54/2.54 = 1[/tex]
Finally, we multiply all the numbers by 3, so that they are all integers.
[tex]C: 1.66 \times 3 \approx 5\\H: 3.33 \times 3 \approx 10\\O: 1 \times 3 = 3[/tex]
The empirical formula of the organic compound is C₅H₁₀O₃.
You can learn more about empirical formula here: https://brainly.com/question/21280037
