Combustion of a 0.1908 g sample of a compound gave 0.2895 g CO₂ and 0.1192 g H₂O. Combustion of a second sample weighing 0.1825 g yielded 40.2 mL of N₂(g), collected over 50% KOH(aq) (vapor pressure = 9 mmHg) at 25 °C and 735 mmHg barometric pressure. When 1.082 g of compound was dissolved in 26.00 g benzene (mp 5.50 °C, K_f = 5.12 °C mol kg^-1), the solution had a freezing point of 3.66 °C. What is the molecular formula of this compound?