Question

K₁ and K₂ are the equilibrium constants for the reactions respectively.

N₂(g)+O₂(g)K₁⇐⇒2NO(g)
2NO(g)+O₂(g)K2⇐⇒2NO₂(g)

What is the equilibrium constant for the required reaction
NO₂(g)⇔1/2N₂(g)+O₂(g)

A. 1/√K₁K₂
B. (K₁=K₂)¹/²
C. 1/2K₁K₂
D. (1/K₁K₂)32

Answer 1

The equilibrium constant for the reaction NO2(g) ⇔ ½N2(g) + O2(g) can be found by taking the inverse of the product of the given equilibrium constants K1 and K2, making the answer D. (1/K1K2)^3.

Step-by-step explanation:

The student is asking how to calculate the equilibrium constant for the reaction NO2(g) ⇔ ½N2(g) + O2(g) given the equilibrium constants K1 and K2 for the two related reactions:

1. N2(g) + O2(g) ⇌ 2NO(g) with an equilibrium constant K1
2. 2NO(g) + O2(g) ⇌ 2NO2(g) with an equilibrium constant K2

To find the equilibrium constant for the reverse reaction of NO2(g) forming ½N2(g) + O2(g), denoted as K', it is important to understand that for the reverse reaction, the equilibrium constant is the inverse of the equilibrium constant of the forward reaction. In this case, we need to calculate (1/K1)*(1/K2) or 1/(K1*K2), which gives us the overall equilibrium constant for the reaction as described by the student. Therefore, the correct answer is D. (1/K1K2)3.