A compound contains only carbon, hydrogen, and oxygen. Combustion of 26.42 g of the compound yields 39.61 g of CO₂ and 10.81 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*

1. Calculate the grams of carbon (C) in 26.42 g of the compound: grams
2. Calculate the grams of hydrogen (H) in 26.42 g of the compound. grams
3. Calculate the grams of oxygen (O) in 26.42 g of the compound. grams

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Based on your previous answers, calculate

1. the moles of carbon (C) in 26.42 g of the compound: moles
2. the moles of hydrogen (H) in 26.42 g of the compound: moles
3. the moles of oxygen (O) in 26.42 g of the compound: moles

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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

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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

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Answer rating: 100% (QA)

C H 3961 g COx 1081 HOx 1 mol CO 4401 g CO 1 mol HO 1802g HO Number of moles of C 4091 g x H Numbe... View the full answer