An unknown compound contains carbon, hydrogen and oxygen. Combustion analy of the compound gives mass percents of \( 31.57 \% \mathrm{C} \) and \( 5.30 \% \mathrm{H} \). The molecular weig is determined by measuring the freezing point depression of an aqueous solution. freezing point of \( -5.20^{\circ} \mathrm{C} \) is recorded for a solution made by dissolving \( 10.56 \mathrm{~g} \) of \( t \) compound in \( 25.0 \mathrm{ml} \) of water. Determine the empirical formula, molecular weig and molecular formula of the compound. \( \mathrm{Ans}: \mathrm{EF}=\mathrm{MF} \mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}_{6} ; \mathrm{MWt}=\mathbf{1 5 2} \mathrm{g} / \mathrm{mol} \)
Added by Michael N B.
Close
Step 1
57% carbon, 5.30% hydrogen, and the rest is oxygen, we can calculate the number of moles of each element in 100g of the compound. For carbon: (31.57g C) / (12.01g/mol) = 2.63 mol C For hydrogen: (5.30g H) / (1.01g/mol) = 5.25 mol H For oxygen: (100g - 31.57g - Show more…
Show all steps
Your feedback will help us improve your experience
Lijeesh Krishnan and 91 other Chemistry 102 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound gives mass percents of $31.57 \%$ C and $5.30 \%$ H. The molar mass is determined by measuring the freezing-point depression of an aqueous solution. A freezing point of $-5.20^{\circ} \mathrm{C}$ is recorded for a solution made by dissolving $10.56 \mathrm{g}$ of the compound in $25.0 \mathrm{g}$ water. Determine the empirical formula, molar mass, and molecular formula of the compound. Assume that the compound is a nonelectrolyte.
An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound gives mass percents of 31.57$\% \mathrm{C}$ and 5.30$\%$ H. The molar mass is determined by measuring the freezing-point depression of an aqueous solution. A freezing point of $-5.20^{\circ} \mathrm{C}$ is recorded for a solution made by dissolving 10.56 $\mathrm{g}$ of the compound in 25.0 $\mathrm{g}$ water. Determine the empirical formula, molar mass, and molecular formula of the compound. Assume that the compound is a nonelectrolyte.
A compound of carbon, hydrogen, and oxygen was burned in oxygen, and $1.000 \mathrm{~g}$ of the compound produced $1.434 \mathrm{~g} \mathrm{CO}_{2}$ and $0.783 \mathrm{~g} \mathrm{H}_{2} \mathrm{O} .$ In another experiment, $0.1107 \mathrm{~g}$ of the compound was dissolved in $25.0 \mathrm{~g}$ of water. This solution had a freezing point of $-0.0894^{\circ} \mathrm{C}$. What is the molecular formula of the compound?
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Watch the video solution with this free unlock.
EMAIL
PASSWORD