What does it mean when K>1, K<1, K=1, and when K=0.   Is your equilibrium constant always constant, or can it change?  Please explain!

Consider the following reaction: A(g) = 3 B(g) A reaction mixture initially contains 1.3 M of A. Determine the equilibrium concentration of B if Kc for the reaction at this temperature is 8.62 x 10. Calculate this based on the assumption that the x value is negligible compared to 1.3.

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

Suppose a 250. mL flask is filled with 1.9 mol of Br,, 1.8 mol of BrOCl and 1.6 mol of BrCl. The following reaction becomes possible: Br, (g) + OC1, (g) = BIOC1(g) + BrC1(g) The equilibrium constant K for this reaction is 4.15 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. 0.53 M ?