The given question is incomplete. The complete question is as follows.
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.
Explanation:
Chemical equation for the oxidation of ammonia is as follows.
Then volume of per second consumed is as follows.
V =
As this reaction is taking place at a temperature of (468.15 K) and pressure 0.88 atm. Hence, moles of consumption of are calculated as follows.
n =
=
= 14.77 mol /sec
When 5 moles of produces 4 moles of NO then the amount of NO produced from 14.77 mol
= 354.60 g/s
Therefore, NO formed per second is as follows.
= 0.35 kg/s
Thus, we can conclude that the rate at which nitrogen monoxide is being produced is 0.35 kg/s.
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Miller collected several organic compounds, both simple (such as formaldehyde) and complex (such as hydrocarbons), commonly found in organisms.
Though his methodology is not undisputed, his results support the concept that abiotic synthesis of organic compounds could have been an early stage in the origin of life.
From the samples collected for chemical analysis, Miller identified a variety of organic molecules that are common in organisms. These included simple compounds, such as formaldehyde (CH2O) and hydrogen cyanide (HCN), and more complex molecules, such as amino acids and long chains of carbon and hydrogen known as hydrocarbons. Miller concluded that organic molecules, a first step in the origin of life, may have been synthesized abiotically on the early Earth.
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