Consider the reactions and their respective equilibrium constants: NO(8) + įBr2(8) = NOB1(g) Kp = 5.3 Kp = 2.1 x 1030 Use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction: 2 NO(g) = N2(g) + O2(g) N2(8) + O2(g) + Brz(3) = 2 NOB1(g)

Carbon monoxide is a colorless, odorless gas that binds irreversibly to hemoglobin in our blood, causing suffocation and death. Co is formed during incomplete combustion of carbon. One way to represent this equilibrium is: 2c0(g)=2 C(s) + 02(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) C(s) + 1/2 02(g)=co(g) K = 2) 2 C(s) + 02(g) =2c0(g) K2 = %3D 3) CO(g) C(s) + 1/2 02(g) K3 = Drag and drop your selection from the following list to complete the answer: 1/K K1/2 (1/K)1/2

For each of the reactions and equilibrium constants below, determine whether the equilibrium mixture will contain mostly products, mostly reactants, a comparable amount of reactants and products, or if is impossible to tell. Reaction Equilibrium Constant Equilibrium mixture  A(g) + 2 B(g) ⇋ 2 C(g) + D(g) 9.4 x 10-8 at 530 K   A(g) + B(g) ⇋ C(g) + D(g)  3.8 x 107 at 340 K    2 A(g) ⇋ C(g) + D(g)  0.8 at 485 K

An equilibrium is established for the reaction 2 CO(g) + MoO2(s) = 2 CO2(g) + Mo(s). Use the expression for Kp from part a. If at equilibrium the partial pressure of carbon monoxide is 5.21 atm and the partial pressure of the carbon dioxide is 0.717 atm, then what is the value of Kp?

Ammonia and oxygen react to form nitrogen and water, like this: 4NH3(g)+30₂(g) → 2N₂(g) + 6H₂O(g) Suppose a mixture of NH3, O₂, N₂ and H₂O has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation Some NH3 is removed. Some N₂ is added. change in composition The pressure of O₂ will The pressure of N₂ will The pressure of NH3 will The pressure of O₂ will ? ? ? ? O O C C shift in equilibrium O to the right Oto the left O (none) X O to the right O to the left O (none) 5 E C

The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K.2SO3(g) 2SO2(g) + O2(g)If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1030 K?Kp =  ---   The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K.PCl3(g) + Cl2(g) PCl5(g)If ΔH° for this reaction is -87.9 kJ, what is the value of Kp at 416 K?Kp =

1 A + 2 B → 2 C Calculate the equilibrium constant (K) for the following reaction at 1000. K, using this information: A and B are placed in a flask and at the beginning of the reaction [A] is 8.95 M and [B] is 6.21 M. After the reaction has reached equilibrium,[B] is 1.94 M. Please ignore significant figures for this problem.

The reaction of hydrazine (N2H4) with chlorine trifluoride (ClF3) has been used in experimental rocket motors.N2H4(g) + 4/3 ClF3(g)  4 HF(g) + N2(g) + 2/3 Cl2(g)   (Kp)How is the equilibrium constant, Kp, for this reaction related to Kp' for the reaction written this way?3 N2H4(g) + 4 ClF3(g)  12 HF(g) + 3 N2(g) + 2 Cl2(g)   (Kp' ) A. 3 Kp = Kp' B. (Kp)3 = Kp' C. Kp = (Kp' )3 D. Kp = Kp'

Consider the synthesis of ammonia: N2(g) + 3H2(g)<=>2NH3(g) At 926.5 °C, the equilibrium constant Kp  is 4.09  × 10–5. What is the value of Kc?

Write the expression for the equilibrium constant Kp for the following reaction.Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3)2 as (P NH3)2 . If either the numerator or denominator is 1, please enter 1   2 Co3O4(s)   ↔   6 CoO(s) + O2(g)           K   =