Nitric oxide (NO) occurs in the atmosphere naturally at a concentration of 0.1 p

Question

Nitric oxide (NO) occurs in the atmosphere naturally at a concentration of 0.1 ppb Determine whether or not this concentration represents equilibrium with respect to H_2O, O_2: and ammonia (NH_3) all in the gaseous phase. Convert the concentration of NO to its partial pressure, assuming an atmospheric pressure of 1 bar Write the appropriate chemical reaction that governs the concentration of NO in the atmosphere if equilibrium were maintained between NO, NH_3. H_2O. and O_2. Important: place O_2 on the right hand side of the reaction. The equilibrium constant for this reaction is 10^84.03. Calculate the partial pressure of NH_3 as if the reaction is controlled by chemical equilibrium. Are the concentrations of NO and NH_3 in the atmosphere a result of chemical equilibrium, explain?

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