Chapter 10, Problem 63QP

Ethanol $\left({\text{C}}_{\text{2}}{\text{H}}_{\text{5}}\text{OH}\right)$ burns in air:

${\text{C}}_{\text{2}}{\text{H}}_{\text{5}}\text{OH(}l{\text{) + O}}_{\text{2}}(g)\underset{}{\to }{\text{CO}}_2(g)+{\text{H}}_2\text{O(}l\text{)}$

Balance the equation and determine the volume of air in liters at $\text{45}\text{.0°C}$ and 793 mmHg required to bum 185 g of ethanol. Assume that air is 21.0 percent ${\text{O}}_{\text{2}}$ by volume.