The equilibrium constant (KP) for the formation of the air pollutant nitric oxide (NO) in an automobile engine at 537°C is 4.5 × 10−11. N2(g) + O2(g) ⇌ 2NO(g) (a) Calculate the partial pressure of NO under these conditions if the partial pressures of nitrogen and oxygen are 3.00 and 0.012 atm, respectively. (b) Repeat the calculation for atmospheric conditions in which the partial pressures of nitrogen and oxygen are 0.78 and 0.21 atm, and the temperature is 25°C. (The KP for the reaction is 4.0 × 10−31 at this temperature.)
The equilibrium constant (KP) for the formation of the air pollutant nitric oxide (NO) in an automobile engine at 537°C is 4.5 × 10−11. N2(g) + O2(g) ⇌ 2NO(g) (a) Calculate the partial pressure of NO under these conditions if the partial pressures of nitrogen and oxygen are 3.00 and 0.012 atm, respectively. (b) Repeat the calculation for atmospheric conditions in which the partial pressures of nitrogen and oxygen are 0.78 and 0.21 atm, and the temperature is 25°C. (The KP for the reaction is 4.0 × 10−31 at this temperature.)
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 36QAP: At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s),...
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The equilibrium constant (KP) for the formation of the air pollutant nitric oxide (NO) in an automobile engine at 537°C is 4.5 × 10−11.
N2(g) + O2(g) ⇌ 2NO(g)
(a) Calculate the partial pressure of NO under these conditions if the partial pressures of nitrogen and oxygen are 3.00 and 0.012 atm, respectively.
(b) Repeat the calculation for atmospheric conditions in which the partial pressures of nitrogen and oxygen are 0.78 and 0.21 atm, and the temperature is 25°C. (The KP for the reaction is 4.0 × 10−31 at this temperature.)
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