The Empirical Formula For Acetic Acid Is CH2O. Its Molar Mass Is 60 G/Mol. The Molecular Formula Is
The Correct Answer and Explanation is :
The molecular formula of acetic acid is C₂H₄O₂.
Explanation:
The empirical formula represents the simplest whole-number ratio of elements in a compound. For acetic acid, the empirical formula is CH₂O, meaning the elements are in a 1:2:1 ratio of carbon, hydrogen, and oxygen.
To determine the molecular formula, we need to compare the empirical formula mass with the given molar mass:
- Calculate the empirical formula mass (CH₂O):
- Carbon (C) = 12 g/mol
- Hydrogen (H) = 1 × 2 = 2 g/mol
- Oxygen (O) = 16 g/mol
- Total = 12 + 2 + 16 = 30 g/mol
- Determine the molecular formula:
- The given molar mass of acetic acid = 60 g/mol
- Divide the molar mass by the empirical formula mass:
[
\frac{60}{30} = 2
] - This means the molecular formula is 2 times the empirical formula:
[
(CH₂O) × 2 = C₂H₄O₂
]
Thus, the correct molecular formula of acetic acid is C₂H₄O₂.
Additional Explanation:
Acetic acid is the main component of vinegar, giving it a sour taste and strong smell. Structurally, it consists of a carboxyl group (-COOH) attached to a methyl group (-CH₃). The molecular formula C₂H₄O₂ accurately represents this structure.
Now, I’ll generate an image representing acetic acid’s molecular structure.
Here is a 3D molecular structure of acetic acid (C₂H₄O₂), showing the carboxyl group (-COOH) and the methyl group (-CH₃) with color-coded atoms. Let me know if you need any modifications or additional explanations!
