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What is the molecular formula of a compound with the impirical formula c4h4o and a molar mass of 136 grams per mole?
To determine the molecular formula from the empirical formula (C4H4O) and the molar mass (136 g/mol), first calculate the molar mass of the empirical formula: C4H4O has a molar mass of 88 g/mol (C: 12 g/mol x 4 + H: 1 g/mol x 4 + O: 16 g/mol). Next, divide the molar mass of the compound by the molar mass of the empirical formula: 136 g/mol ÷ 88 g/mol = 1.545, which rounds to 1.5. Since we cannot have a fractional ratio in molecular formulas, we multiply the empirical formula by 3 to get C12H12O3, which matches the molar mass of 136 g/mol. Therefore, the molecular formula is C12H12O3.
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What is the molecular formula for the unknown C2H4O?
That is a molecular formula.I can't off the top of my head think of any compound with that molecular formula, though. It's not methoxyethane or a propanol, because it's got one too few hydrogen atoms. It's not propanone or cyclopropanol or oxetane or a propenol, because it's got one too many hydrogen atoms.
What is the empirical formula of C16H16O4?
C4H4O - you just divide everything by the highest common factor (4 in this case)
What is the molecular formula for the unknown C2H4O?
That is a molecular formula.I can't off the top of my head think of any compound with that molecular formula, though. It's not methoxyethane or a propanol, because it's got one too few hydrogen atoms. It's not propanone or cyclopropanol or oxetane or a propenol, because it's got one too many hydrogen atoms.
What is the empirical formula of C16H16O4?
C4H4O - you just divide everything by the highest common factor (4 in this case)
