A compound contains only carbon, hydrogen, and oxygen. Combustion of 86.30 g of

Question

A compound contains only carbon, hydrogen, and oxygen. Combustion of 86.30 g of the compound yields 129.4 g of CO2 and 35.31 g of H2O. The molar mass of the compound is 176.1 g/mol. *Each part of this problem should be submitted separately to avoid losing your work* Calculate the grams of carbon (C) in 86.30 g of the compound: grams Calculate the grams of hydrogen(H) in 86.30 g of the compound: grams Calculate the grams of oxygen(O) in 86.30 g of the compound: grams Based on your previous answers, calculate the moles of carbon (C) in 86.30g of the compound: moles calculate the moles of hydrogen (H) in 86.30g of the compound: moles calculate the moles of oxygen(O) in 86.30g of the compound: moles

Explanation / Answer

86.3 produces 129.4 gm of CO2 176.1 produces = 264.05 gms of CO2 86.3 produces 35.31 gm of H2O 176.1 produces = 72.05 gms of CO2 moles of CO2 = 264.05 / mm of CO2 = 6 moles 0f H2O = 72.05 / mm of H2O = 4 it means compound has 6 atoms of carbon 8 atoms of hydrogen and rest oxygen no. of oxygen atoms = (176/1 - )/16 = 6 hence compound is C6H8O6 a) 1) gms of carbon = 3*12=36 2) gms of hydrogen = 2*1 = 2 3)gms of oxygen = 3* 16 = 48 b) 1) moles of carbon = 3 2) moles of hydrogen = 2 3) moles of oxygen = 3

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