[lelouch]

The catalyzed combustion of ammonia is one of the steps in the manufacture of nitric acid. The reaction involves the oxidation of NH3 (molar mass = 17 g / mol) with gaseous oxygen. They are produced mononitrogênio monoxide (nitric oxide) and water vapor. Suppose air containing 80% nitrogen and 20% oxygen by volume is used in the reaction and the speed of air consumption is 56 m³ / min, measured at STP (0 degrees Celsius and ATM), a reactor that operates a 100% yield. Under these conditions, the amount of ammonia consumed in 1 hour of reactor operation is?: "

result: 408 kg

I explain how to answer this.

[Borek]

Simple stoichiometry. Start with the reaction equation, calculate amount of oxygen consumed per hour, calculate amount of ammonia that will react with this oxygen. Bingo.

[lelouch]

Thank you. I was a mess. I got to do now.