Question

The combustion of 40.5 mg of a compound containing $C$, $\mathrm{H},$ and $\mathrm{O},$ and extracted from the bark of the sassafras tree, produces $110.0 \mathrm{mg}$ of $\mathrm{CO}_{2}$ and $22.5 \mathrm{mg}$ of $\mathrm{H}_{2} \mathrm{O} .$ The molar mass of the compound is $162 \mathrm{g} / \mathrm{mol}$. Determine its empirical and molecular formulas.

Name: The combustion of 40.5 mg of a compound containing C, H, and O, and extracted from the bark of the sassafras tree, produces 110.0 mg of CO2 and 22.5 mg of H2O . The molar mass of the compound is 162 g / mol. Determine its empirical and molecular formulas.
Uploaded: 2023-03-14T06:17:38-08:00
Duration: 1 min 52 s
Channel: Adi S
Description: The combustion of 40.5 mg of a compound containing C, H, and O, and extracted from the bark of the sassafras tree, produces 110.0 mg of CO2 and 22.5 mg of H2O . The molar mass of the compound is 162 g / mol. Determine its empirical and molecular formulas.

          The combustion of 40.5 mg of a compound containing $C$, $\mathrm{H},$ and $\mathrm{O},$ and extracted from the bark of the sassafras tree, produces $110.0 \mathrm{mg}$ of $\mathrm{CO}_{2}$ and $22.5 \mathrm{mg}$ of $\mathrm{H}_{2} \mathrm{O} .$ The molar mass of the compound is $162 \mathrm{g} / \mathrm{mol}$. Determine its empirical and molecular formulas.

Added by Joshua O.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

03/14/2023

Step 1

Moles of CO2 = mass / molar mass = 110.0 mg / (44.01 g/mol) = 0.00250 mol Moles of H2O = mass / molar mass = 22.5 mg / (18.02 g/mol) = 0.00125 mol Show more…

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The combustion of 40.5 mg of a compound containing $C$, $\mathrm{H},$ and $\mathrm{O},$ and extracted from the bark of the sassafras tree, produces $110.0 \mathrm{mg}$ of $\mathrm{CO}_{2}$ and $22.5 \mathrm{mg}$ of $\mathrm{H}_{2} \mathrm{O} .$ The molar mass of the compound is $162 \mathrm{g} / \mathrm{mol}$. Determine its empirical and molecular formulas.