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AnnZ [28]
3 years ago
10

An unknown organic compound composed of carbon, hydrogen, and oxygen was analyzed and found to be 50.84% C, 8.53% H, and the res

t oxygen. What is the empirical formula
Chemistry
1 answer:
MariettaO [177]3 years ago
7 0

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.

C =  \frac{50.84}{12} = 4.24 mol

For Hydrogen.

H =  \frac{8.53}{1} = 8.53 mol

For Oxygen.

O =  \frac{40.63}{16} = 2.54 mol

Step 2: Divide each of the numbers by the smallest number.

For Carbon.

C =  \frac{4.24}{2.54} = 1.7

For Hydrogen.

H =  \frac{8.53}{2.54} = 3.36

For Oxygen.

O =  \frac{2.54}{2.54} = 1

Step 3: So the empirical formula will be.

C_{1.7} H_{3.36} O_1

But using decimal will be messy. So we multiply the numbers by 3. The right empirical formula will be.

C_{5} H_{10} O_3

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