Question

Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 908. liters per second of dioxygen are consumed when the reaction is run at 235.°C and 0.92atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits.

Answer 1