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March 28, 2017

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0.717 g of a compound containing carbon, hydrogen, and oxygen is burned and found to produce 1.02 g CO2 and 0.624 g H2O. The molar mass of the compound is 124 g/mol.
(a) Write a chemical equation for the combustion of this unknown hydrocarbon.
(b) Determine the # of g and moles of carbon, hydrogen, and oxygen in the unknown hydrocarbon.
(c) Calculate the empirical formula.
(d) Calculate the molecular formula.
(e) Write the balanced equation for the combustion reaction.

  • Chemistry - ,

    You must know SOMETHING about this problem. Tell me what you know and I can help you through the remainder of it.

  • Chemistry - ,

    You know the mass of the hydrocarbon and the what mass of the products produced are as well as the mass of the compound.

  • Chemistry - ,

    part b. Convert g CO2 to g C, convert g H2O to g hydrogen, add the two and subtract from 0.717 to find g oxygen. Then I would find %C, %H, and %O. Take a 100 g sample and find moles. moles = grams/molar mass.

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