Chapter 11, Problem 11.138MP

A compound that contains only C and H was burned in excess O₂ to give CO₂ and H₂O. When 0.270 g of the compound was burned, the amount of CO₂ formed reacted completely with 20.0 mL of 2.00 M NaOH solution according to the equation

$\text{2}{\text{OH}}^{-}\text{(}aq\text{)}+{\text{CO}}_{\text{2}}(g)\stackrel{}{\to }{\text{CO}}_{\text{3}}{{}^2}^{-}\text{(}aq\text{)}+{\text{H}}_{\text{2}}\text{O}\left(l\right)$

When 0.270 g of the compound was dissolved in 50.0 g of camphor, the resulting solution had a freezing point of 177.9 °C. [Pure camphor freezes at 179.8 °C and has K_f = 37.7 (°C · kg)/mol.]

1. (a) What is the empirical formula of the compound?
2. (b) What is the molecular weight of the compound?
3. (c) What is the molecular formula of the compound?