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- Directions: Analyze each item and identify the molecular formula of the compound. 7. The percentage composition of acetic acid is found to be 39.9% C, 6.7% H, and53.4% O. Determine the empirical and molecular formula of acetic acid if the molarmass is 60.0g/mol.8. Determine the molecular formula of the compound with an empirical formula of CHand a formula mass of 78g/mol.9. Aniline has an empirical formula of C6H7N, what is the molecular formula if its molaris 93g/mol?10. What’s the empirical formula of a molecule containing 65.5% carbon, 5.5%hydrogen, and 29.0% oxygen? If the molar mass of the compound is 110grams/mole, what’s the molecular formula?points A 0.1938 g of an organic compound known to contain C and H only was burned. The traps for H2O and CO₂ increased in mass by 0.2750 g and 0.5972 g. respectively. What is the percentage of carbon?Question 2. Calculate the molecular weight of Freon-12, if 122.70 liters of its vapor at 200 °C and 790 mm HG has a mass of 397 g. Show your work.
- Lysine is an amino acid which has the following elemental composition: C, H, O, N. Inone experiment, 2.175 g of lysine was combusted to produce 3.94 g of CO2 and 1.89 gH2O. In a separate experiment, 1.873 g of lysine was burned to produce 0.436 g of NH3.The molar mass of lysine is approximately 150 g/mol. Determine the empirical andmolecular formula of lysineGeneral formula of a polymer is-(CH2CHCHCN)n-, where n is typically greater than 10,000. Then take a sample of this polymer weighs 755.9 g and contains 3.112 x 1020 molecules of -(CH2CHCHCN)n-, so calculate n?What is the mass percent of carbon in isopropyl alcohol, C3H8O? Group of answer choices 40.0% 60.0% 25.0% 20.0% 26.6%
- 14 what is the name and molar mass of this structure?For the following table fill in the missing values and calculate the theoretical yield. A + 2B à C moles 0.00242 0.00242 ?_________ MW ?_________ 98.06 164.16 g ?_________ ?__0.00002467_______ ?_________ mL 0.20 d(g/mL) 0.80A hydrocarbon compound (containing only H and C) is completely combusted in excess oxygen gas. If 0.440 g and 0.180 g of carbon dioxide (44.0 g/ mol) and water (18.0 g/mol) are created respectively, which formula below would be possible? C2H5 C2H4 C2H2 C2H6 C6H6
- hello, does 12◦C not included in the formula? and how does it become 9.12 x 10 raise to negative 2?Please display on how to do the problem step by step: Combustion of 8.732 mg of an unknown organic compound gave 16.432 mg of CO2and 2.840 mg of H2O. (a) Find the wt% of C and H in the substance. (b) Find the smallest integer mole ratio of C:H in the compound.A hydrate [hydrates have the general formula AB • xH2O] is found to have the percentcomposition: Na = 19.17%, C = 10.00%, H = 4.17% and O = 66.6%. After heating to 100 oC todrive off the water of hydration, the percent composition is found to be: Na = 27.38%,C = 14.28%, H = 1.19% and O = 57.15%. From this data, determine the probable molecularformula for the hydrate if the molecular weight = 120 amu.