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Solved: At 1000 K, a sample of pure NO2 gas decomposes:
Chapter 14, Problem 42P(choose chapter or problem)
At 1000 K, a sample of pure \(\mathrm{NO}_{2}\) gas decomposes:
\(2 \mathrm{NO}_{2}(g)\ \leftrightharpoons\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)\)
The equilibrium constant \(K_{P}\) is 158. Analysis shows that the partial pressure of \(\mathrm{O}_{2}\) is 0.25 atm at equilibrium. Calculate the pressure of NO and \(\mathrm{NO}_{2}\) in the mixture.
Questions & Answers
QUESTION:
At 1000 K, a sample of pure \(\mathrm{NO}_{2}\) gas decomposes:
\(2 \mathrm{NO}_{2}(g)\ \leftrightharpoons\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)\)
The equilibrium constant \(K_{P}\) is 158. Analysis shows that the partial pressure of \(\mathrm{O}_{2}\) is 0.25 atm at equilibrium. Calculate the pressure of NO and \(\mathrm{NO}_{2}\) in the mixture.
ANSWER:Step 1 of 2
The decomposition reaction is shown below.
Given,
The equilibrium constant, 
The partial pressure of oxygen is 0.25 atm.