In the reaction below, a mixture of carbon monoxide, hydrogen, and methanol is at equilibrium at 250°C. The mixture contains 0.0960 M CO, 0.191 M H2, and 0.150 M CH3OH. What is the value for Kc? CO( 9) + 2 H2( g) = CH3OH(g) Enter your answer to 2 significant figures.

Consider the following reaction: SO₂Cl2 (g) SO₂ (g) + Cl₂ (g) A reaction mixture is made containing an initial [SO₂Cl₂] of 2.4×10-2 M. At equilibrium, [Cl₂] = 1.3×10-² M. Part A Calculate the value of the equilibrium constant (Kc). Express your answer to two significant figures.

Initial (M) Change (M) Equilibrium (M) Consider the reaction of SO₂ and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO₂(g) + O₂(g) = 2 SO₂(g) NEXT A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂ at 900 K and allowed to react. At equilibrium, the concentration of SO, was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. -0.00875 0.0209 0 0.00875 2SO₂(g) Question 20 of 33 2.00 0.0216 0.0432 0.0148 0.0296 0.0041 O₂(g) 0.0175 2 0.0129 -0.0175 0.0061 RESET -0.0350 0.0257 2SO₂(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 = ???