A compound containing C, H, N, and O is burned in excess oxygen. The gases produced by burning 0.1152 g are first treated to convert the nitrogen-containing product gases into N₂, and then the resulting mixture of CO₂, H₂O, N₂, and excess O₂ is passed through a bed of CaCl₂ to absorb the water. The CaCl₂ increases in mass by 0.09912 g. The remaining gases are bubbled into water to form H₂CO₃, and this solution is titrated with 0.3283 M NaOH; 28.81 mL is required to achieve the second equivalence point. The excess O₂ gas is removed by reaction with copper metal (to give CuO). Finally, the N₂ gas is collected in a 225.0-mL flask, where it has a pressure of 65.12 mm Hg at 25°C. In a separate experiment, the unknown compound is found to have a molar mass of 150 g/mol. What are the empirical and molecular formulas of the unknown compound?