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 Tries 0/99 Based on your previous answers, calculate the moles of carbon (C) in 86.30 g of the compound: moles calculate the moles of hydrogen (H) in 86.30 g of the compound: moles calculate the moles of oxygen (O) in 86.30 g of the compound: moles Tries 0/99 Divide each mole quantity that you determined in the previous question by the smallest number of moles to determine the correct empirical formula. Enter the correct subscript for each atom using the smallest whole number. Enter a 1 if that is the smallest whole number, don't leave the box empty. C H O Tries 0/99 Now determine the molecular formula. Remember that the molar mass of the compound is 176.1 g/mol. Enter the correct subscript for each atom using the smallest whole number. Enter a 1 if that is the smallest whole number, don't leave the box empty. C H O Tries 0/99

Explanation / Answer

1)35.2 2)3.9 3)125.61

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