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A compound contains only carbon, hydrogen, and oxygen. Combustion of 26.12 g of the compound yields 38.29 g of CO2 and 15.67 g of H₂O. The molar mass of the compound is 90.078 g/mol. *Each part of this problem should be submitted separately to avoid losing your work* 1. Calculate the grams of carbon (C) in 26.12 g of the compound: 2. Calculate the grams of hydrogen (H) in 26.12 g of the compound. 3. Calculate the grams of oxygen (O) in 26.12 g of the compound. Submit Answer Tries 0/10 Based on your previous answers, calculate 1. the moles of carbon (C) in 26.12 g of the compound: 2. the moles of hydrogen (H) in 26.12 g of the compound: 3. the moles of oxygen (O) in 26.12 g of the compound: Submit Answer Tries 0/10 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 Submit Answer Tries 0/10 Divide each mole quantity that you determined in the previous question by the smallest number of moles to determine the correct empirical formula. moles moles moles H Submit Answer Tries 0/10 O grams grams grams H Now determine the molecular formula. Remember that the molar mass of the compound is 90.078 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 O