The statements in the tables below are about two different chemical equilibria. The symbols have their usual meaning, for example AG stands for the standard Gibbs free energy of reaction and K stands for the equilibrium constant. In each table, there may be one statement that is false because it contradicts the other three statements. If you find a false statement, check the box next to it. Otherwise, check the "no false statements" box under the table. statement In K>0 K>1 AG <0 AS"> AH* T no false statements false? O O O O O statement AG">0 AH" T AS <3 Ink<0 K>1 no false statements false? O O O O O B

Methanol liquid burns readily in air. One way to represent this equilibrium is: CH₂OH(1) + 3/2 0₂(g) CO₂(g) + 2 H₂O(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) 2 CH₂OH(1) + 3 O₂(g) 2) 2 CO₂(g) + 4H₂O(g) 2 CO₂(g) + 4H₂O(g) 2 CH₂OH(1) + 3 O₂(g) CH₂OH(1) + 3/2 0₂(g) K3 K₁ = K₂ = 3) CO₂(g) + 2 H₂O(g) Drag and drop your selection from the following list to complete the answer: K² (1/K)² 1/K

1. Given the equilibrium constant values N₂ (g) + ¹/2O₂(g) → N₂O (g) N₂O4 (g) → 2 NO₂ (g) ½ N₂(g) + O₂(g) → NO₂ (g) Kel=2.7 x 10-18 K₂=4.6 x 10-³ K3 = 4.1 x 10⁹ Determine the value of K. for the reaction below: 2 N₂O(g) + 30₂ (g) → 2 N₂O4 (g)

Please find the equilibrium constant (K) for reaction "3" below by using any/all of the information presented below.  Note, I will use <-> to indicate equilibrium arrows Rxn 1     2 NO(g) <-> N2(g) +O2(g)                K1= 2.1x1030 Rxn 2     2 NO(g) +Br2(g) <-> 2 NOBr(g)       K2 = 28.09 Rxn 3     N2(g) +Br2(g) +O2(g) <-> 2 NOBr(g)    K = ???