The equilibrium constant (Kp) for the formation of the air pollutant nitric oxide (NO) in an automobile engine at 530 degree C is 2.9 x 10 to the minus eleventh
N2(g) + O2 (g) = 2 NO (g)
What is the partial pressure of NO under these conditions if the partial pressures of nitrogen and oxygen are 3.0 atm and 0.013 atm, respectively ?
What is it for atmospheric conditions where the partial pressures of nitrogen and oxygen are 0.78 atm and 0.18 atm and the temperature is 25 degrees C ?( Kp= 4.0 x 10 to the minus 31 at this temperature)
Is the formation of NO endothermic or exothermic?
Using the formation constant Kp of NO, the partial pressure of gas is calculated. Also, the formation is classified as a endothermic process based on the equilibrium constant at different temperature.