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Complete combustion of 10.69 g of a compound of carbon, hydrogen, and oxygen yielded 13.56 g CO₂ and 3.703 g H₂O. When 16.60 g of the compound was dissolved in 318 g of water, the freezing point of the solution was found to be -0.933 °C. For water, Kfp = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O

Complete combustion of 10.69 g of a compound of carbon, hydrogen, and oxygen yielded 13.56 g CO₂ and 3.703 g H₂O. When 16.60 g of the compound was dissolved in 318 g of water, the freezing point of the solution was found to be -0.933 °C. For water, Kfp = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter12: Solutions
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Problem 12.55QE
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Complete combustion of 10.69 g of a compound of carbon, hydrogen, and oxygen yielded 13.56 g CO₂ and 3.703 g H₂O. When 16.60 g of the compound was dissolved in 318 g of water, the freezing point of the solution was found to be -0.933 °C. For water, Kfp = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O molecular formula =
Transcribed Image Text:Complete combustion of 10.69 g of a compound of carbon, hydrogen, and oxygen yielded 13.56 g CO₂ and 3.703 g H₂O. When 16.60 g of the compound was dissolved in 318 g of water, the freezing point of the solution was found to be -0.933 °C. For water, Kfp = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O molecular formula =
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