Chapter 5, Problem 80E

Urea (H₂NCONH₂) is used extensively as a nitrogen source in fertilizers. It is produced commercially from the reaction of ammonia and carbon dioxide:

$2{\text{NH}}_{\text{3}}\left(g\right)+{\text{CO}}_{\text{2}}\left(g\right)\underset{\text{Pressure}}{\overset{\text{Heat}}{\to }}{\text{ H}}_{\text{2}}{\text{NCONH}}_{\text{2}}\left(s\right)+{\text{ H}}_{\text{2}}\text{O}\left(g\right)$

Ammonia gas at 223°C and 90. atm flows into a reactor at a rate of 500. L/min. Carbon dioxide at 223°C and 45 atm flows into the reactor at a rate of 600. L/min. What mass of urea is produced per minute by this reaction assuming 100% yield?