N2(g) + O2(g) reversible 2NO (g) If the equillibrium partial pressures of N2, O2

Question

N2(g) + O2(g) reversible 2NO (g) If the equillibrium partial pressures of N2, O2, and NO are 0.15 atm, 0.33 atm and 0.050 atm, respectively at 2200 C, what is Kp?
N2(g) + O2(g) reversible 2NO (g) If the equillibrium partial pressures of N2, O2, and NO are 0.15 atm, 0.33 atm and 0.050 atm, respectively at 2200 C, what is Kp?
N2(g) + O2(g) reversible 2NO (g) If the equillibrium partial pressures of N2, O2, and NO are 0.15 atm, 0.33 atm and 0.050 atm, respectively at 2200 C, what is Kp?
If the equillibrium partial pressures of N2, O2, and NO are 0.15 atm, 0.33 atm and 0.050 atm, respectively at 2200 C, what is Kp?

Explanation / Answer

Kp for the reaction as :

kp = [NO]2 / [N2] [O2]

putting all the values we get :

Kp = (0.050)2 / (0.15) (0.33)

= 0.05

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