Chapter 26, Problem 81IAE

Combustion of a 0.1908 g sample of a compound gave 0.2895 g $C{O}_2$ and 0.1192 g $H_{2}O$ .Combustion of a second sample weighing 0.1825 g yielded 40.2 mL of $N_2$ (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 $(mp5.50°C,K_f=5.12°Cmo{l}^{}k{g}^{-1})$ , the solution had a freezing point of 3.66 $°C$ . What isthe molecular formula of this compound?