N2 (g) + O2 (g) =2 NO (g) Describe a step-by-step method to calculate the equilibrium concentration of NO when the initial concentrations [N2] = 0.12 M, [O2] = 0.12 M, [NO] = 1.45 M The equilibrium constant for the reaction is Kp = 5.0 x 10 2. %3D Be sure to first convert Kp to Kc, then use an ICE table to determine the equilibrium concentration of NO.

Aluminum metal and bromine liquid (red) react violently to make aluminum bromide (white powder). One way to represent this equilibrium is: 2 AlBr3(s)2 Al(s) + 3 Br2(1) 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) AIBr3(s) PAl(s) + 3/2 Br2(1) K1 = 2) Al(s) + 3/2 Br2(1) AlBr3(s) K2 = 3)2 Al(s) + 3 Br2(1) =2 AIBR3(s) K3 = Drag and drop your selection from the following list to complete the answer: (1/K)1/2 K/2 1/K

A mixture 0.600 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium concentration of COBr2 was 0.25 M. What is the value of Kc for this reaction? (Write your answer with 3 significant figures)CO(g) + Br2(g) ↔  COBr2(g)

Consider the following reaction where K. = 10.5 at 350 K: 2 CH;Cl2 (g)=CH4 (g)+ CCI4 (g) A reaction mixture was found to contain 1.10x10-2 moles of CH,Cl, (g), 4.63×10-2 moles of CH4 (g), and 3.70×10² moles of CCl (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: v 1. In order to reach equilibrium CH,Cl,(g) must be produced. v 2. In order to reach equilibrium K, must decrease v 3. In order to reach equilibrium CH, must be consumed. v 4. Qc is greater than K. 5. The reaction is at equilibrium. No further reaction will occur. T