A 27.0 g sample of an unknown hydrocarbon compound (containing carbon and hydrogen only) was burned in excess oxygen to form 88.0 g of CO2 and 27.0 g of H2O. Identify which of the following is a possible molecular formula for the hydrocarbon. C4H6CH4C2H6C6H6

A 2.554-g sample of a certain hydrocarbon is burned in excess oxygen, producing 8.635 g CO2(g) and 1.768 g H2O(l). If the molecular weight of the hydrocarbon is found to be 78.11 u, what is its molecular formula? [m.w. CO2 = 44.01 u; m.w. H2O = 18.02 u]

A 4.235 g sample of a hydrocarbon was burned in oxygen to give 3.810 g of H2O and 13.96 g of CO2. What is the empirical formula of the compound?

A compound is found to contain 24.0 g carbon, 4.00 mol hydrogen and 1.204 × 1024 atoms of oxygen. What is the empirical formula of this compound? CH2OC2H4O2CH2O2C2H4O

An organic molecule contains 70.6% Carbon, 5.9% Hydrogen and 23.5% Oxygen. It has a molecular mass of 136. What is its chemical formula? A. C4H4O B. C5H4O C. C8H8O2 D. C10H8O2 E. C2H2O

An organic acid contains 41.4% carbon, 3.47% hydrogen, and 55.1% oxygen by mass. A 0.050 mol sample of this compound weighs 5.80 g. What is the molecular formula of this acid? CHO C6H6O6 C3H3O C2H2O2 C4H4O4