Solution: Consider the following reactions and their respective equilibrium constants:NO(g) + 1/2 Br2(g) ⇌ NOBr(g); Kp = 5.32 NO(g) ⇌ N2(g) + O2(g); Kp = 2.1 x 1030Use these reactions and their equilibrium cons

Consider the following reactions and their respective equilibrium constants:
NO(g) + 1/2 Br₂(g) ⇌ NOBr(g); K_p = 5.3
2 NO(g) ⇌ N₂(g) + O₂(g); K_p = 2.1 x 10³⁰

Use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction:
N₂(g) + O₂(g) + Br₂(g) ⇌ 2 NOBr(g)