Determine the correct empirical formula of a compound containing 26.68% carbon, 2.24% hydrogen, and 71.08% oxygen.

The correct empirical formula of a compound containing 26.68% carbon, 2.24% hydrogen, and 71.08% oxygen is CHO₂

The empirical formulae shows us how elements in a compound are in their simplest ratio.

From the question, we can see  

Carbon (C) with  26.68%

Hydrogen (H)with  2.24%

Oxygen (O) with 71.08%

Now, the empirical formula of the compound can begotten following these steps:

Carbon  = 26.68 /12 = 2.223

Hydrogen= 2.24 / 1 = 2.24

Oxygen  = 71.08 / 16 = 4.4425

C arbon = 2.223 / 2.223 = 1

H ydrogen= 2.24 / 2.223 = 1

Oxygen  = 4.4425 /2.223 = 2

Giving us the empirical formula of the compound as CHO₂

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CHO₂

Explanation:

The following data were obtained from the question:

Carbon (C) = 26.68%

Hydrogen (H) = 2.24%

Oxygen (O) = 71.08%

Empirical formula =?

The empirical formula of the compound can be obtained as follow:

C = 26.68%

H = 2.24%

O = 71.08%

Divide by their molar mass.

C = 26.68 /12 = 2.223

H = 2.24 / 1 = 2.24

O = 71.08 / 16 = 4.4425

Divide by the smallest.

C = 2.223 / 2.223 = 1

H = 2.24 / 2.223 = 1

O = 4.4425 /2.223 = 2

Thus the empirical formula of the compound is CHO₂