Question

An organic compound contains carbon = 38.71%, Hydrogen = 9.67% and Oxygen. The empirical formula of the compound would be:

• A. \( CH_3O \)
• B. \( CH_4O \)
• C. \( CH_2O \)
• D. \( CHO \)

Hint:

The empirical formula represents the simplest whole-number ratio of atoms in a compound. Use the percentages of elements to calculate their molar ratios.

Answer 1

The Correct Option is C

To find the empirical formula, we first assume a 100 gm sample. Thus, the percentages become grams: - Carbon: 38.71 gm - Hydrogen: 9.67 gm - Oxygen: 100 - 38.71 - 9.67 = 51.62 gm Now, we divide the grams of each element by their atomic mass: - Carbon: \( \frac{38.71}{12} = 3.23 \) - Hydrogen: \( \frac{9.67}{1} = 9.67 \) - Oxygen: \( \frac{51.62}{16} = 3.23 \) The simplest whole number ratio is approximately 1:2:1, which gives the empirical formula \( CH_2O \).