# Question #b830c

Mar 5, 2017

66.24g ${O}_{2}$

#### Explanation:

We use the density of the 1-propanol to find its mass, and from that the number of moles. Then we can use the reaction equation to compare the number of moles of propanol reacted to the number of moles of oxygen consumed.. We can then convert those moles of ${O}_{2}$ into its mass.

17.21mL * 0.803 g/mL = 13.82g ${C}_{3} {H}_{7} O H$ 13.82g/60g/mol = 0.23 moles of 1-propanol.

From the equation, 1 mole 1-propanol reacts with 9 moles of ${O}_{2}$. Therefore, 0.23 moles will require 2.07 moles of ${O}_{2}$.
2.07mol * 32g/mol = 66.24g ${O}_{2}$