Chemistry, 12.03.2020 00:40 aniacopenowell7
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 645. liters per second of dioxygen are consumed when the reaction is run at 195.oC and 0.88 atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.
Answers: 3
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Areaction is first order with respect to reactant x and second order with respect to reactant y. which statement describes the rate law for this reaction?
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Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first...
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