Consider the following reactions and their respective equilibrium constants: NO (g) + ½ Brz (g) NOBI (g) K1 = 5.3 2 NO (g) + 02 (g)= N204 (g) K2 = 2.1 x 10-5 N204 (g) = N2 (g) + 2 O2 (g) K3 = 4.8 x 1025 se reactions and their equilibrium constants to predict the equilibrium constant for owing reaction: N2 (g) + O2 (g) + Br2 (g) 2 NOB1 (g)

Suppose that for a hypothetical reaction: A2(g) + 3B2(g) 2 2AB3(g) It is determined that at a certain temperature the equilibrium concentrations are [A] =0.0040, [B2] = 0.746 and [AB3] = 6.7x10 Calculate the numerical value of K for the reaction. K =

12) If 1.34 moles each of Br2 and Cl2 are introduced into an 11.0 liter flask and allowed to come to equilibrium, what should the equilibrium concentrations of Br2, Cl2, and BrCl be? 2 BrCl (g) « Br2 (g) + Cl2 (g)​​​Kc = 0.143

Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react according to the following reaction. PCI3(g)+ Cl2(g) = PCl5(g) The equilibrium constant for the reaction is Kc, = 37.5 at 145 °C. If 0.222 mol of phosphorus trichloride is added to 0.750 mol of chlorine in a 1.69 - L reaction vessel and allowed to react at this temperature, what is the equilibrium concentration (in mol/L) of phosphorus pentachloride? Report your answer to THREE significant figures.

3. If the equilibrium constant K, for the reaction 2 NO (g) + O2(g) = 2 NO2 (g) is 5.0 x 1012 at a given temperature, what is the value of the equilibrium constant K, for each of the following reactions at the same temperature? a) NO (g) + ½ O2 (g) → NO2 (g) b) 2 NO2 (g) = 2 NO (g) + 02 (g) c) NO2(g) = NO (g) + ½ 02 (g)

Consider the reaction: P(s) + 3/2Cl₂ (g) → PC13 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: P(s) + 5/2Cl₂ (g) ⇒ PCl5(9) K₁ PC13 (g) + Cl2 (g) PC15 (9) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter K² if the first equilibrium constant should be squared. K =

At a particular temperature, K = 1.00 x 10² for the reaction H₂(g) +1₂(g) → 2HI(g) In an experiment, 1.00 mol H₂, 1.00 mol 12, and 1.00 mol HI are introduced into a 1.00 L container. Calculate the equilibrium concentrations of all reactants and products.

Nitrogen oxides are air pollutants produced by the reaction of nitrogen and oxygen at high temperatures. At 2000 °C, the value of the equilibrium constant for the reaction, N2(g)+O2(g)=2NO(g), is 4.1 x 10-4. Find the concentration of NO(g) in an equilibrium mixture with air at 1 atm pressure at this temperature. In air, [N,] = 0.036 mol/L and [O,] 0.0089 mol/L.

The equilibrium constant, Kc, is given for one of the reactions below. What is the value of the missing equilibrium constant, Kc? Cl₂(g) + H₂O(g) = 2 HCl(g) + 1/2 O₂(g) K = 7.52 × 10-2 4 HCI(g) + O₂(g) = 2 Cl₂(g) + 2 H₂O(g) OK= 5.66 x 10-3 OK= 13.3 OK= 0.150 OK = 177 OK = 3.65 K = ?

Cyclohexane, C6H12, a hydrocarbon, can isomerize or change into methylcyclopentane, a compound of the same formula (C5 H9 CH3) but with a different molecular structure. Cyclohexane Methylcyclopentane The equilibrium constant has been estimated to be 0.12 at 25 °C. If you had originally placed 0.053 mol of cyclohexane in a 2.8 L flask, what would be the concentrations of cyclohexane and methylcyclopentane when equilibrium is established? [cyclohexane] = M [methylcyclopentane] = M