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 liters per second of oxygen are consumed when the reaction is run at and . Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Round your answer to significant digits.