Consider the following equilibrium, 2 NO (g) N ₂(g) + O ₂(g); K_ C₁ = 2.4 10²⁰ NO (g) + 1 2 Br ₂(g) NOBr (g); K_ C₂ = 1.4 Calculate K_C for the reaction, 1 2 N ₂(g) + 1 2 O ₂(g) + 1 2 Br ₂(g) NOBr (g)

Step-by-step solution

Target reaction: 1 2 N₂(g) + 1 2 O₂(g) + 1 2 Br₂(g) NOBr(g) Reverse reaction 1 and multiply by 1 2 : 1 2 N₂(g) + 1 2 O₂(g) NO(g) , K'' = 1 K₁ = 1 2.4 10²⁰ Add reaction 2 as it is: NO(g) + 1 2 Br₂(g) NOBr(g) , K₂ = 1.4 K_C = K'' K₂ = 1.4 2.4 10²⁰ = 1.4 2.4 10¹⁰ = 1.4 0.64 10¹⁰ 0.896 10¹⁰ = 8.96 10⁻¹¹