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13 Dec 2019

A compound of C, H, and O was burned in oxygen, and 1.000 g ofthe compound produced 1.418 g CO2 and .871 g H2O. In anotherexperiment, .1103 g of the compound was dissolved in 45.0 g ofwater. This solution had a freezing point of -.0734 degrees C. Whatis the molecular formula of the compound?

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Beverley Smith
Beverley SmithLv2
17 Dec 2019
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Related questions

I have been working on this question. I do not know wheretostart. Could you please show me how to start and work throughthisquestion? I beleive its a delta change of freezing pointdepressionquestion, and im pretty sure that you have to figure outthemolarity of all the compounds in the molecular formula, yet imnotsure what effect burning has on the problem. Futhermore,Iunderstand its a multiple step problem and it is reallyconfusingme.
Here is the question:
A compound of carbon, hydrogen, and oxygen was burnedinoxygen, and 1.000g of the compound produced 1.418 g CO2 and .871gH2O. In another experiment, .1103 g of the compound wasdissolvedin 45.0 g of water. This solution had a freezing point of-0.0734degrees C. What is the molecular formula of thecompound?
Help!

Complete combustion of 12.34 g of a compound of carbon, hydrogen, and oxygen yielded 21.99 g CO2 and 9.005 g H2O. When 11.40 g of the compound was dissolved in 323 g of water, the freezing point of the solution was found to be -0.889 °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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